Mass and gaseous volume relationships in chemical reactionsTopic 1 – Quantitative Chemistry

Reacting masses

•Stoichiometry

•Combustion of methane

Mass Conversions (the world of stoichiometry)•__Al (s) + __I2 (s) __AlI3 (s)•35.0 g of Al will react with how many

grams of I so there is no excess reactant?•Step 1 convert known into moles•Step 2 convert moles of known into

moles of unknown•Step 3 convert moles of unknown into

grams of unknown

Example

•10.00 grams of sodium hydroxide is reacted with excess sulfuric acid in the following reaction:▫2NaOH(s) + H2SO4(aq) Na2SO4(aq) + H2O(l)

▫What mass of Na2SO4 · 7H2O is produced?

example

•Sodium hydrogen carbonate decomposes into sodium carbonate, water, and carbon dioxide when heated. How much Sodium hydrogen carbonate is needed to produce 8.80 g of CO2?

example

•How much oxygen gas is required for the complete combustion of .250 mol. of propane gas (C3H8)?

example

•Solid lithium hydroxide is used to remove carbon dioxide from the environment. The products are solid lithium carbonate and liquid water. What mass of carbon dioxide can 1.00 x 103 g of lithium hydroxide absorb? How much water is produced?

Example 3

•Baking soda (NaHCO3) and Milk of magnesia are antacids to neutralize excess HCl in the stomach

•Balanced equations:▫NaHCO3(s) + HCl(aq) NaCl(aq) + H2O(l) + CO2(g)

▫Mg(OH)2(s) + 2HCl (aq) 2H2O(l) + MgCl2(s)

•Which antacid is better?

Limiting reactants

•Methane reacts with water to produce hydrogen gas and carbon monoxide

•What quantity of water is required to react exactly with 249g of methane?

•What if you have 300.g of water

Limiting Reactant

•What if there are not exact combinations of reactants?

•One reactant will run out before the other is used up

•One reactant is in excess•The limiting factor is what determines the

amount of product that can be formed

Example

•Ammonia is an important fertilizer to farmers and is produced by combining nitrogen gas and hydrogen gas. If you have 25.0 kg of nitrogen gas is reacted with 5.00 kg of hydrogen gas. How much ammonia is going to be produced?

Steps to solve

•Step 1 – when in doubt convert to moles

•Step 2 – Determine the limiting reactant

•Step 3 – calculate the mass of product using the limiting reactant

Example

•Nitrogen gas can be created by passing gaseous ammonia over solid copper (II) oxide at high temps. Other products formed are solid copper and water vapor.

•If you have 18.1g of NH3 and 90.4 g of CuO. How many grams of Nitrogen can be produced?

Do we get all that product?

•Why?

•Percent yield = actual yield / theoretical yield

•If in the last problem you actually obtained 6.63 g of nitrogen what was the percent yield of the reaction?

Example

•68.5 kg of CO(g) is reacted with 8.60 kg of H2(g) to form methanol (CH3OH). What is the theoretical yield? If you actually produce 3.57x104 g what is the percent yield?

Example

•Lithium nitride is prepared by the reaction of lithium metal and nitrogen gas. Calculate the amount of lithium nitride formed when 56.0 g of lithium react with 56.0 g of nitrogen.

Example •Titanium (IV) oxide is a solid white used as a

coloring pigment is made by reacting gaseous titanium (IV) chloride with oxygen gas. Chlorine gas is also formed as a by-product. If 6.71x103 g of titanium (IV) chloride is reacted with 2.45x103 g of oxygen, how much titanium (IV) oxide can be produced? If the percent yield is 75.0%, how much titanium (IV) oxide was actually produced?

Avogadro’s laws in gasses

•Avogadro’s hypothesis – at a standard temperature and pressure all gasses will occupy 22.4 dm3 mol-1. (STP = 1 atm & 273K)

•2CO2(g) + O2(g) 2CO2(g)

Calculations

•10 cm3 of ethyne is reacted with 50 cm3 of hydrogen to produce ethane in the following equation:▫C2H2(g) + H2(g) C2H6(g)

▫Calculate the volume of the ethane gas, and any remaining reactant.

Molar volume of a gas

•Mol of a gas = Volume of gas / molar volume

•Calculate the number of moles and mass of oxygen gas in 5.00 dm3 of oxygen at STP.

example

•What mass of sodium hydrogen carbonate must be heated to create 10.00 dm3 of carbon dioxide at STP?

•What volume of air (20% oxygen) is needed to completely combust 1.000 kg of gasoline (C3H8) at STP?

Ideal gas

Boyle’s lawVolume pressure P x V

48.0 29.1

40.0 35.3

32.0 44.2

24.0 58.2

Examples•What is the new volume of 1.5 L sample of

Freon –12 at 56 torr compressed to 150 torr?

•In an automobile the initial volume of an engine cylinder is .725 L and an initial pressure of 1 atm. If the piston is moved to a volume of .075 L what will the new pressure be?

Charles’s Law

Example

•A 2.0 L sample of air is collected at 298 K and cooled to 278 K, what is the new volume?

•A gas has an original volume of .675L and a temp. of 35.0 oC. If the volume is changed to .535 L what is the temperature of the gas?

Lussac’s Law

Combined gas law

•A syringe contains 50 cm3 of gas at 1.0 atm and 20.0oC is heated to 100.0oc and changed to 5.0 atm.▫What is the new volume?

Ideal Gas Law•All of the gas law constants can be

combined to help create a general equation

•What are all the laws thus far?•R is the gas constant•R = .0821 when P is atm and V is L•Use the ideal gas law when gas is at 1

condition•Works best when gas is at low pressure

(1atm or less) and higher temp (above 0oC)•Equation PV=nRT

Example

•A sample of hydrogen gas has a volume of 8.56 L at 0oC and a pressure of 1.5 atm. How many moles of hydrogen are there? Molecules of Hydrogen?

Example II

•What volume is occupied by .250 mol of carbon dioxide at 25oC and .488 atm?

Example III

•.240 mol sample of ammonia at 25oC with a volume of 3.5 L and a pressure of 1.68 atm. The gas is compressed to a volume of 1.35 L What is the final pressure