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Chapter 11

Gases

Laurie LeBlancCuyamaca College

Clicker Questions

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A. The volume occupied by a gas is mostly empty space.B. The average kinetic energy of the gas particles is

proportional to the temperature in Celsius.C. The attraction/repulsion between gas molecules is very

weak or negligible.D. Gas molecules or atoms move in a straight line between

collisions.E. All of the above are correct postulates.

All of the following are postulates of the kinetic molecular theory of gases EXCEPT:

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A. The volume occupied by a gas is mostly empty space.B. The average kinetic energy of the gas particles is

proportional to the temperature in Celsius.C. The attraction/repulsion between gas molecules is very

weak or negligible.D. Gas molecules or atoms move in a straight line between

collisions.E. All of the above are correct postulates.

All of the following are postulates of the kinetic molecular theory of gases EXCEPT:

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A. 0.76 atmB. 1.00 atmC. 5.80 atmD. 0.763 atmE. 4.41 × 105 atm

Convert 580 mm Hg to units of atmospheres.

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A. 0.76 atmB. 1.00 atmC. 5.80 atmD. 0.763 atmE. 4.41 × 105 atm

Convert 580 mm Hg to units of atmospheres.

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A. 2.41 kPaB. 2.45 × 102 kPaC. 5.29 × 102 kPaD. 2.45 × 105 kPaE. 5.29 × 105 kPa

Convert 35.5 psi to kPa. (Note: 1 atm = 14.7 psi; 1 atm = 101,325 Pa)

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Convert 35.5 psi to kPa. (Note: 1 atm = 14.7 psi; 1 atm = 101,325 Pa)

A. 2.41 kPaB. 2.45 × 102 kPaC. 5.29 × 102 kPaD. 2.45 × 105 kPaE. 5.29 × 105 kPa

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A. × 1B. × 2C. × 4D. × 1/2E. × 1/4

A gas has a volume of 1.0 L at 1 atm. By what factor must the pressure change in order to reduce the volume by half? (Assume the temperature is constant.)

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A. × 1B. × 2C. × 4D. × 1/2E. × 1/4

A gas has a volume of 1.0 L at 1 atm. By what factor must the pressure change in order to reduce the volume by half? (Assume the temperature is constant.)

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A. 651 mLB. 1.65 × 103 mLC. 0.151 mLD. 151 mLE. 500. mL

A flask with 500.0 mL of a gas is sealed on top of Mt. Everest where the atmospheric pressure is 230. torr. What is the volume of the gas when the bottle is moved to sea level at a constant temperature?

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A. 651 mLB. 1.65 × 103 mLC. 0.151 mLD. 151 mLE. 500. mL

A flask with 500.0 mL of a gas is sealed on top of Mt. Everest where the atmospheric pressure is 230. torr. What is the volume of the gas when the bottle is moved to sea level at a constant temperature?

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A. –273 °FB. The freezing point of hydrogenC. The x-intercept of a straight-line graph of V versus 1/PD. The x-intercept of a straight-line graph of V versus TE. The temperature of deep outer space

What is absolute zero?

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A. –273 °FB. The freezing point of hydrogenC. The x-intercept of a straight-line graph of V versus 1/PD. The x-intercept of a straight-line graph of V versus TE. The temperature of deep outer space

What is absolute zero?

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A. 0.375 LB. 0.959 LC. 1.20 LD. 0.833 LE. 1.88 L

A flexible container contains 1.50 L of gas at 25 °C. What is the new volume when the container is heated to 100 °C at a constant pressure?

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A. 0.375 LB. 0.959 LC. 1.20 LD. 0.833 LE. 1.88 L

A flexible container contains 1.50 L of gas at 25 °C. What is the new volume when the container is heated to 100 °C at a constant pressure?

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A. 0.740 gB. 11.8 gC. 0.740 molD. 23.7 gE. None of the above

A 36.1 mL sample of oxygen gas contains 0.529 mol of oxygen. If enough oxygen is added to the sample to obtain a volume of 50.5 mL, what must the final mass of the sample be? (The pressure and temperature is constant.)

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A. 0.740 gB. 11.8 gC. 0.740 molD. 23.7 gE. None of the above

A 36.1 mL sample of oxygen gas contains 0.529 mol of oxygen. If enough oxygen is added to the sample to obtain a volume of 50.5 mL, what must the final mass of the sample be? (The pressure and temperature is constant.)

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A. Avogadro’s B. Charles’sC. Dalton’s D. Gay-Lussac’sE. Boyle’s

What law is derived from the combined gas law under constant temperature and moles?

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A. Avogadro’s B. Charles’sC. Dalton’s D. Gay-Lussac’sE. Boyle’s

What law is derived from the combined gas law under constant temperature and moles?

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A. 1.00 molB. 2.00 molC. 3.00 molD. 5.00 molE. 10.0 mol

A container with 1.00 mol of gas is expanded from 5.00 L to 10.0 L by adding more gas. How many moles of gas are present? (The temperature and pressure are kept constant.)

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A. 1.00 molB. 2.00 molC. 3.00 molD. 5.00 molE. 10.0 mol

A container with 1.00 mol of gas is expanded from 5.00 L to 10.0 L by adding more gas. How many moles of gas are present? (The temperature and pressure are kept constant.)

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A. 37.8 psiB. 35.0 psiC. 0 psiD. 40.1 psiE. 29.9 psi

A set of car tires contains a volume of 45.5 L of air at 35.0 psi and 0.0 °C. When the car is driven, the temperature of the tires increases to 40.0 °C. What is the pressure (in psi) of each tire, assuming constant volume?

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A. 37.8 psiB. 35.0 psiC. 0 psiD. 40.1 psiE. 29.9 psi

A set of car tires contains a volume of 45.5 L of air at 35.0 psi and 0.0 °C. When the car is driven, the temperature of the tires increases to 40.0 °C. What is the pressure (in psi) of each tire, assuming constant volume?

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A. 1.3 molB. 0.229 molC. 0.174 molD. 2.58 molE. 0.17 mol

How many moles of an ideal gas are in a container with a volume of 5.5 L at 580 mm Hg and 20. °C?

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A. 1.3 molB. 0.229 molC. 0.174 molD. 2.58 molE. 0.17 mol

How many moles of an ideal gas are in a container with a volume of 5.5 L at 580 mm Hg and 20. °C?

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A. 0.0295 LB. 1.00 LC. 22.4 LD. 48.8 LE. 0.0446 L

What is the volume occupied by 28.0 g of nitrogen gas at 1.00 atm and 0.0 °C?

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A. 0.0295 LB. 1.00 LC. 22.4 LD. 48.8 LE. 0.0446 L

What is the volume occupied by 28.0 g of nitrogen gas at 1.00 atm and 0.0 °C?

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A. H2

B. N2

C. F2

D. O2

E. Cl2

A 4.17 g sample of a diatomic gas at 38 °C has a volume of 1.5 L at 1.00 atm. Identify the gas.

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A. H2

B. N2

C. F2

D. O2

E. Cl2

A 4.17 g sample of a diatomic gas at 38 °C has a volume of 1.5 L at 1.00 atm. Identify the gas.

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A. when both the pressure and temperature are high.B. when the pressure is high and the temperature is low.C. when both the pressure and temperature are low.D. when the pressure is low and the temperature is high.E. Real gases have ideal behavior no matter what the

conditions are.

A real gas can approach ideal behavior

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A. when both the pressure and temperature are high.B. when the pressure is high and the temperature is low.C. when both the pressure and temperature are low.D. when the pressure is low and the temperature is high.E. Real gases have ideal behavior no matter what the

conditions are.

A real gas can approach ideal behavior

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A. 2.02 g/molB. 4.00 g/molC. 28.0 g/molD. 32.0 g/molE. 38.1 g/mol

Calculate the molar mass of a gas that has a density of 1.70 g/L at STP.

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A. 2.02 g/molB. 4.00 g/molC. 28.0 g/molD. 32.0 g/molE. 38.1 g/mol

Calculate the molar mass of a gas that has a density of 1.70 g/L at STP.

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A. 5.00%, 70.3%, 24.7%B. 6.67%, 66.0%, 27.3% C. 0.500%, 49.5%, 50.0%D. 10.0%, 50.0%, 40.0%E. 1.50%, 75.5%, 23.0%

The partial pressures in a mixture of CO2, N2, and O2 in a sample of gas are 50.0 atm, 495 atm, and 205 atm, respectively. Calculate the mole percentage of each gas.

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A. 5.00%, 70.3%, 24.7%B. 6.67%, 66.0%, 27.3% C. 0.500%, 49.5%, 50.0%D. 10.0%, 50.0%, 40.0%E. 1.50%, 75.5%, 23.0%

The partial pressures in a mixture of CO2, N2, and O2 in a sample of gas are 50.0 atm, 495 atm, and 205 atm, respectively. Calculate the mole percentage of each gas.

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A. 9 mm HgB. 69 mm HgC. 626 mm HgD. 635 mm HgE. 644 mm Hg

A sample of hydrogen gas is collected over water at a pressure of 635 mm Hg at 10.0 °C. Calculate the partial pressure of hydrogen. (The vapor pressure of water at 10.0 °C is 9.2 mm Hg.)

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A. 9 mm HgB. 69 mm HgC. 626 mm HgD. 635 mm HgE. 644 mm Hg

A sample of hydrogen gas is collected over water at a pressure of 635 mm Hg at 10.0 °C. Calculate the partial pressure of hydrogen. (The vapor pressure of water at 10.0 °C is 9.2 mm Hg.)

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A. 0.225 LB. 36.3 LC. 201 LD. 403 LE. 0.0239 L

How many liters of oxygen gas are produced by the complete decomposition of 225 mL of water? The oxygen gas is collected at 580. torr and 27 °C. (The density of water at 27 °C is 1.00 g/mL)

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A. 0.225 LB. 36.3 LC. 201 LD. 403 LE. 0.0239 L

How many liters of oxygen gas are produced by the complete decomposition of 225 mL of water? The oxygen gas is collected at 580. torr and 27 °C. (The density of water at 27 °C is 1.00 g/mL)

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A. 0.705 gB. 2.82 gC. 12.7 gD. 38.1 gE. 50.8 g

How many grams of water are produced from the complete combustion of 15.8 L of propane (C3H8) gas at STP?

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A. 0.705 gB. 2.82 gC. 12.7 gD. 38.1 gE. 50.8 g

How many grams of water are produced from the complete combustion of 15.8 L of propane (C3H8) gas at STP?

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A. 1.00 mol O2

B. 48.0 g O2

C. 0.500 mol HeD. 4.008 g H2

E. 6.02 × 1023 molecules of N2

Which of the following samples occupy the largest volume at STP?

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A. 1.00 mol O2

B. 48.0 g O2

C. 0.500 mol HeD. 4.008 g H2

E. 6.02 × 1023 molecules of N2

Which of the following samples occupy the largest volume at STP?

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A. V and PB. T and PC. V and TD. V and nE. None of the above

For an ideal gas, which two variables are inversely proportional to each other, assuming all the other conditions remain constant?

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A. V and PB. T and PC. V and TD. V and nE. None of the above

For an ideal gas, which two variables are inversely proportional to each other, assuming all the other conditions remain constant?

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A. increases by a factor of 75.B. halves.C. doubles.D. remains the same.E. None of the above

At a constant pressure, when the temperature of a gas sample is doubled from 75 °C to 150 °C, the volume of the gas

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A. increases by a factor of 75.B. halves.C. doubles.D. remains the same.E. None of the above

At a constant pressure, when the temperature of a gas sample is doubled from 75 °C to 150 °C, the volume of the gas

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A. Avogadro’s lawB. Boyle’s lawC. Charles’s lawD. Gay-Lussac’s lawE. Dalton’s Law

Which of the following gas laws relate volume and temperature?

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Which of the following gas laws relate volume and temperature?

A. Avogadro’s lawB. Boyle’s lawC. Charles’s lawD. Gay-Lussac’s lawE. Dalton’s Law

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A. PaB. atmC. mm HgD. torrE. psi

What is the SI unit for pressure?

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A. PaB. atmC. mm HgD. torrE. psi

What is the SI unit for pressure?

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A. 369 °CB. 25.0 °CC. 96.8 °CD. 2.47 °CE. 9.68 °C

A 158 mL sample of gas has a pressure of 0.989 atm and a temperature of 25.0 °C. What is the final temperature (°C) when the pressure increases to 1.01 atm and the volume decreases to 192 mL?

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A. 369 °CB. 25.0 °CC. 96.8 °CD. 2.47 °CE. 9.68 °C

A 158 mL sample of gas has a pressure of 0.989 atm and a temperature of 25.0 °C. What is the final temperature (°C) when the pressure increases to 1.01 atm and the volume decreases to 192 mL?

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A. 1.38 atmB. 8.85 atmC. 5.68 atmD. 0.989 atmE. 1.27 atm

If a 7.45 L sample of nitrogen at STP is compressed to a volume of 5.81 L and warmed to 295 K, what is the final pressure of the sample?

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A. 1.38 atmB. 8.85 atmC. 5.68 atmD. 0.989 atmE. 1.27 atm

If a 7.45 L sample of nitrogen at STP is compressed to a volume of 5.81 L and warmed to 295 K, what is the final pressure of the sample?

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A. 0.072 atmB. 695 mm HgC. 125 mm HgD. 55 mm HgE. Two of the above

A mixture of nitrogen, hydrogen, and oxygen has a total pressure of 695 mm Hg. If the partial pressure of nitrogen is 435 mm Hg and the partial pressure of hydrogen is 205 mm Hg, what is the partial pressure of oxygen?

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A. 0.072 atmB. 695 mm HgC. 125 mm HgD. 55 mm HgE. Two of the above

A mixture of nitrogen, hydrogen, and oxygen has a total pressure of 695 mm Hg. If the partial pressure of nitrogen is 435 mm Hg and the partial pressure of hydrogen is 205 mm Hg, what is the partial pressure of oxygen?

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A. 22.4 LB. 45 LC. 720 mLD. 130 mLE. 20. L

Water decomposes to form hydrogen and oxygen gases. What volume of oxygen gas measured at 750 mm Hg and 35 °C is formed when 28 g of water is reacted?

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A. 22.4 LB. 45 LC. 720 mLD. 130 mLE. 20. L

Water decomposes to form hydrogen and oxygen gases. What volume of oxygen gas measured at 750 mm Hg and 35 °C is formed when 28 g of water is reacted?

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A. 0.1115 gB. 7.9 gC. 1.295 gD. 7.904 gE. 3.953 g

What is the mass of a sample of chlorine gas that occupies a volume of 2.500 L at STP?

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A. 0.1115 gB. 7.9 gC. 1.295 gD. 7.904 gE. 3.953 g

What is the mass of a sample of chlorine gas that occupies a volume of 2.500 L at STP?