38
The Behavior of Gases • AW Chapter 10, section 1 and Chapter 12
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The Behavior of Gases
bull AW Chapter 10 section 1 and Chapter 12
Gas Pressure
ndash Changing altitude
Atmospheric Pressure
Measuring Gas Pressure
bull A barometer measures atmospheric pressure
bull The barometer was invented by Evangelista Torricelli
in 1643
Measuring Gas Pressure
bull A manometer measures the pressure of a gas in a container
Units of Gas Pressure
1 standard atmosphere
= 1000 atm
= 7600 mm Hg
= 7600 torr
= 101325 kPa
Partial Pressure
bull Partial pressure is the contribution each gas in a mixture makes to the total pressure
Daltonrsquos Law of Partial Pressures
bull For a mixtures of gases in a container the total pressure exerted is the sum of the partial pressures of the gases present
bull Ptotal = P1 + P2 + P3
Daltonrsquos Law of Partial Pressures
bull The pressure is independent of the nature of the particles
bull The pressure of the gas is affected by the number of particles
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull Total pressure is the pressure of the gas + the vapor pressure of the water
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull How can we find the pressure of the gas collected alone
bull Robert Boylersquos
experiment
Pressure and Volume Boylersquos Law
bull Graphing Boylersquos
results This graph
has the shape of
half of a hyperbola
with an equation PV = k
Pressure and Volume Boylersquos Law
Boylersquos Lawbull For a given mass of gas at constant
temperature the volume of a gas varies inversely with pressurendash If one increases the other decreases
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Gas Pressure
ndash Changing altitude
Atmospheric Pressure
Measuring Gas Pressure
bull A barometer measures atmospheric pressure
bull The barometer was invented by Evangelista Torricelli
in 1643
Measuring Gas Pressure
bull A manometer measures the pressure of a gas in a container
Units of Gas Pressure
1 standard atmosphere
= 1000 atm
= 7600 mm Hg
= 7600 torr
= 101325 kPa
Partial Pressure
bull Partial pressure is the contribution each gas in a mixture makes to the total pressure
Daltonrsquos Law of Partial Pressures
bull For a mixtures of gases in a container the total pressure exerted is the sum of the partial pressures of the gases present
bull Ptotal = P1 + P2 + P3
Daltonrsquos Law of Partial Pressures
bull The pressure is independent of the nature of the particles
bull The pressure of the gas is affected by the number of particles
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull Total pressure is the pressure of the gas + the vapor pressure of the water
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull How can we find the pressure of the gas collected alone
bull Robert Boylersquos
experiment
Pressure and Volume Boylersquos Law
bull Graphing Boylersquos
results This graph
has the shape of
half of a hyperbola
with an equation PV = k
Pressure and Volume Boylersquos Law
Boylersquos Lawbull For a given mass of gas at constant
temperature the volume of a gas varies inversely with pressurendash If one increases the other decreases
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Measuring Gas Pressure
bull A barometer measures atmospheric pressure
bull The barometer was invented by Evangelista Torricelli
in 1643
Measuring Gas Pressure
bull A manometer measures the pressure of a gas in a container
Units of Gas Pressure
1 standard atmosphere
= 1000 atm
= 7600 mm Hg
= 7600 torr
= 101325 kPa
Partial Pressure
bull Partial pressure is the contribution each gas in a mixture makes to the total pressure
Daltonrsquos Law of Partial Pressures
bull For a mixtures of gases in a container the total pressure exerted is the sum of the partial pressures of the gases present
bull Ptotal = P1 + P2 + P3
Daltonrsquos Law of Partial Pressures
bull The pressure is independent of the nature of the particles
bull The pressure of the gas is affected by the number of particles
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull Total pressure is the pressure of the gas + the vapor pressure of the water
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull How can we find the pressure of the gas collected alone
bull Robert Boylersquos
experiment
Pressure and Volume Boylersquos Law
bull Graphing Boylersquos
results This graph
has the shape of
half of a hyperbola
with an equation PV = k
Pressure and Volume Boylersquos Law
Boylersquos Lawbull For a given mass of gas at constant
temperature the volume of a gas varies inversely with pressurendash If one increases the other decreases
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Measuring Gas Pressure
bull A manometer measures the pressure of a gas in a container
Units of Gas Pressure
1 standard atmosphere
= 1000 atm
= 7600 mm Hg
= 7600 torr
= 101325 kPa
Partial Pressure
bull Partial pressure is the contribution each gas in a mixture makes to the total pressure
Daltonrsquos Law of Partial Pressures
bull For a mixtures of gases in a container the total pressure exerted is the sum of the partial pressures of the gases present
bull Ptotal = P1 + P2 + P3
Daltonrsquos Law of Partial Pressures
bull The pressure is independent of the nature of the particles
bull The pressure of the gas is affected by the number of particles
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull Total pressure is the pressure of the gas + the vapor pressure of the water
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull How can we find the pressure of the gas collected alone
bull Robert Boylersquos
experiment
Pressure and Volume Boylersquos Law
bull Graphing Boylersquos
results This graph
has the shape of
half of a hyperbola
with an equation PV = k
Pressure and Volume Boylersquos Law
Boylersquos Lawbull For a given mass of gas at constant
temperature the volume of a gas varies inversely with pressurendash If one increases the other decreases
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Units of Gas Pressure
1 standard atmosphere
= 1000 atm
= 7600 mm Hg
= 7600 torr
= 101325 kPa
Partial Pressure
bull Partial pressure is the contribution each gas in a mixture makes to the total pressure
Daltonrsquos Law of Partial Pressures
bull For a mixtures of gases in a container the total pressure exerted is the sum of the partial pressures of the gases present
bull Ptotal = P1 + P2 + P3
Daltonrsquos Law of Partial Pressures
bull The pressure is independent of the nature of the particles
bull The pressure of the gas is affected by the number of particles
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull Total pressure is the pressure of the gas + the vapor pressure of the water
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull How can we find the pressure of the gas collected alone
bull Robert Boylersquos
experiment
Pressure and Volume Boylersquos Law
bull Graphing Boylersquos
results This graph
has the shape of
half of a hyperbola
with an equation PV = k
Pressure and Volume Boylersquos Law
Boylersquos Lawbull For a given mass of gas at constant
temperature the volume of a gas varies inversely with pressurendash If one increases the other decreases
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Partial Pressure
bull Partial pressure is the contribution each gas in a mixture makes to the total pressure
Daltonrsquos Law of Partial Pressures
bull For a mixtures of gases in a container the total pressure exerted is the sum of the partial pressures of the gases present
bull Ptotal = P1 + P2 + P3
Daltonrsquos Law of Partial Pressures
bull The pressure is independent of the nature of the particles
bull The pressure of the gas is affected by the number of particles
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull Total pressure is the pressure of the gas + the vapor pressure of the water
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull How can we find the pressure of the gas collected alone
bull Robert Boylersquos
experiment
Pressure and Volume Boylersquos Law
bull Graphing Boylersquos
results This graph
has the shape of
half of a hyperbola
with an equation PV = k
Pressure and Volume Boylersquos Law
Boylersquos Lawbull For a given mass of gas at constant
temperature the volume of a gas varies inversely with pressurendash If one increases the other decreases
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Daltonrsquos Law of Partial Pressures
bull For a mixtures of gases in a container the total pressure exerted is the sum of the partial pressures of the gases present
bull Ptotal = P1 + P2 + P3
Daltonrsquos Law of Partial Pressures
bull The pressure is independent of the nature of the particles
bull The pressure of the gas is affected by the number of particles
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull Total pressure is the pressure of the gas + the vapor pressure of the water
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull How can we find the pressure of the gas collected alone
bull Robert Boylersquos
experiment
Pressure and Volume Boylersquos Law
bull Graphing Boylersquos
results This graph
has the shape of
half of a hyperbola
with an equation PV = k
Pressure and Volume Boylersquos Law
Boylersquos Lawbull For a given mass of gas at constant
temperature the volume of a gas varies inversely with pressurendash If one increases the other decreases
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Daltonrsquos Law of Partial Pressures
bull The pressure is independent of the nature of the particles
bull The pressure of the gas is affected by the number of particles
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull Total pressure is the pressure of the gas + the vapor pressure of the water
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull How can we find the pressure of the gas collected alone
bull Robert Boylersquos
experiment
Pressure and Volume Boylersquos Law
bull Graphing Boylersquos
results This graph
has the shape of
half of a hyperbola
with an equation PV = k
Pressure and Volume Boylersquos Law
Boylersquos Lawbull For a given mass of gas at constant
temperature the volume of a gas varies inversely with pressurendash If one increases the other decreases
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull Total pressure is the pressure of the gas + the vapor pressure of the water
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull How can we find the pressure of the gas collected alone
bull Robert Boylersquos
experiment
Pressure and Volume Boylersquos Law
bull Graphing Boylersquos
results This graph
has the shape of
half of a hyperbola
with an equation PV = k
Pressure and Volume Boylersquos Law
Boylersquos Lawbull For a given mass of gas at constant
temperature the volume of a gas varies inversely with pressurendash If one increases the other decreases
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Collecting a gas over water
Daltonrsquos Law of Partial Pressures
bull How can we find the pressure of the gas collected alone
bull Robert Boylersquos
experiment
Pressure and Volume Boylersquos Law
bull Graphing Boylersquos
results This graph
has the shape of
half of a hyperbola
with an equation PV = k
Pressure and Volume Boylersquos Law
Boylersquos Lawbull For a given mass of gas at constant
temperature the volume of a gas varies inversely with pressurendash If one increases the other decreases
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
bull Robert Boylersquos
experiment
Pressure and Volume Boylersquos Law
bull Graphing Boylersquos
results This graph
has the shape of
half of a hyperbola
with an equation PV = k
Pressure and Volume Boylersquos Law
Boylersquos Lawbull For a given mass of gas at constant
temperature the volume of a gas varies inversely with pressurendash If one increases the other decreases
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
bull Graphing Boylersquos
results This graph
has the shape of
half of a hyperbola
with an equation PV = k
Pressure and Volume Boylersquos Law
Boylersquos Lawbull For a given mass of gas at constant
temperature the volume of a gas varies inversely with pressurendash If one increases the other decreases
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Boylersquos Lawbull For a given mass of gas at constant
temperature the volume of a gas varies inversely with pressurendash If one increases the other decreases
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Boylersquos Law
Another way of stating Boylersquos Law is
P1V1 = P2V2
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
bull Graphing data
for several gases
Volume and Temperature Charlesrsquos Law
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
bull It is easier to write an equation for the relationship if the lines intersect the origin of the graph
Charlesrsquos Law
ndash Use absolute zero
for the temperature
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Charlesrsquos Law
bull The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
V1 = V2 T1 T2 (where T is in kelvins)
ndash If one increases the other increases
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Pressure and TemperatureGay Lussacrsquos Law
bull The pressure of a fixed mass of gas is directly proportional to its Kelvin temperature if the volume is held constant
P1 = P2
T1 T2
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Pressure Volume and Temperature
Combined Gas Law
bull The three laws Boylersquos Charlesrsquos and Gay Lussacrsquos laws can be combined into a single expression called the combined gas law
P1V1 = P2V2
T1 T2
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Volume and Moles of GasAvogadrorsquos Principle
The volume of a fixed mass of gas is directly proportional to the number of moles of gas if the pressure and temperature are kept constant
V1 = V2 n1 n2
(n = moles of gas)
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Avogadrorsquos Principle
bull If one increases the other increases
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Pressure Volume Temperature and Moles of GasGeneral Gas Law
bull Combining Boylersquos Charlesrsquos Gay Lussacrsquos laws and Avogadrorsquos principle gives the general gas law
P1V1 = P2V2
n1T1 n2T2
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Solve the General Gas Law using data for any gas at standard conditions (STP)
P = 1 atm V = 224 L
n = 1 mole of gas T = 0oC (or 273 K)
P1V1 = (1 atm)(224 L) = 00821 Latm
n1T1 (1 mol)(273 K) Kmol
00821 Latm is the Ideal Gas Constant (R)
Kmol
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
The Ideal Gas Law
P1V1 = R = 00821 L atm
n1T1 mol K
Rearranging the equation gives the ideal gas law
PV = nRT
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Explaining the Ideal Gas Law
Increasing the temperature of agas increases the number of collisions with the container and the force of the collisions so the pressure increases
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Explaining the Ideal Gas Law
Increasing the concentration of agas increases the number of collisions with the container so the pressure Increases (concentration does not affect the force of the collisions)
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Explaining the Ideal Gas Law
Decreasing thevolume of a gas increases the number of collisions with the container so the pressure Increases (volume changes do not affect the force of the collisions)
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Ideal Behavior of GasesThe Kinetic Molecular Theory
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Implications of the Kinetic Molecular
Theory bull Meaning of temperature ndash Kelvin temperature is directly
proportional to the average kinetic energy of the gas particles
bull Relationship between Pressure and Temperature ndash gas pressure increases as the temperature increases because the particles speed up
bull Relationship between Volume and Temperature ndash volume of a gas increases with temperature because the particles speed up
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
bull Gases do not behave ideally under conditions of high pressure and low temperature
bull Why
Real Gases
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
bull At high pressure the volume is decreased ndash Molecule volumes become important ndash Attractions become important
Real Gases
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Diffusion and Effusion of a Gas
bull Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
bull Effusion is the process in which a gas escapes through a tiny hole in its container
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Diffusion and Effusion of a Gas Grahamrsquos Law
bull The rate of diffusion or effusion of a gas is inversely proportional to the square root of the gasrsquos molar mass
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
Grahamrsquos Law Questionhellipbull If a cotton ball with NH3 is placed into one end of a long
glass tube and a cotton ball with HCl is placed into the other end a ring of solid NH4Cl will form where the vapors meet inside the tube
NH3(g) + HCl(g) NH4Cl(solid)
NH3 HCl
a) b) c)
Where will the white ring of NH4Cl form in the tube
Location a b or c
bull Since the HCl is so large in mass it moves more slowly through the tube
bull Since the HCl is so large in mass it moves more slowly through the tube
