Download Name: Date: Performances of Understanding:

Name: _______________________
Date: _______________________
Learning Target:
I can perform stoichiometric calculations, including
determination of mass and volume relationships between
reactants and products for reactions involving gases.
I can describe and calculate the relations between volume,
pressure, number of moles, and temperature for an ideal gas
as described by the ideal gas law.
Criteria for Success:
I can use volume ratios and the gas laws to calculate
volumes, masses, or molar amounts of gaseous reactants or
products.
Performances of Understanding:
-I will listen attentively while completing sample
stoichiometry calculations with the instructor.
-I will self-assess my understanding of the learning
target using my Qwizdom remote.
Guided Practice
1-2. Propane, C3H8, is a gas that is sometimes used as fuel for cooking and heating. The complete combustion of
propane occurs according to the following equation.
C3H8(g) + 5O2(g) → 3CO2(g) +4H2O(g)
1. What will be the volume, in liters, of oxygen required for the complete combustion of 0.250L of propane?
Assume that all volume measurements are made at the same temperature and pressure.
2. What will be the volume of carbon dioxide produced in the reaction? Assume that all volume
measurements are made at the same temperature and pressure.
3. Solid calcium carbonate, also known as limestone, will decompose upon heating to produce solid calcium oxide, also
known as lime (an industrial chemical with a wide variety of uses), and carbon dioxide gas. How many grams of calcium
carbonate must be decomposed to produce 5.00L of carbon dioxide gas at STP? (Note that volume ratios do not apply
here because calcium carbonate is a solid).
4. Tungsten, W, a metal used in light-bulb filaments, is produced industrially by the reaction of tungsten oxide with
hydrogen.
WO3(s) + 3H2(g) → W(s) + 3H2O(g)
How many liters of hydrogen gas at 35°C and 0.980atm are needed to react completely with 875g of tungsten oxide?
Unit Ten 19
Independent Practice
5. Assuming all volume measurements are made at the same temperature and pressure, what volume of hydrogen gas is
needed to react completely with 4.55L of oxygen gas to produce water vapor?
6. Aqueous nitric acid, HNO3, can be produced by the reaction of gaseous nitrogen dioxide with water at room
temperature. Nitrogen monoxide gas is the only other product. If 708L of NO2 gas react with water, what volume of NO
gas will be produced? Assume the gases are measured under standard temperature and pressure conditions.
7. What mass of sulfur must be used to produce 12.61L of gaseous sulfur dioxide at STP according to the following
equation?
S8(s) + 8O2(g) → 8SO2(g)
8. Aluminum granules are a component of some drain cleaners because they react with sodium hydroxide to release
both heat and gas bubbles, which help clear the drain clog. The reaction is
2NaOH(aq) + 2Al(s) + 6H2O(l) → 2NaAl(OH)4(aq) + 3H2(g)
What mass of aluminum would be needed to produce 4.00L of hydrogen gas at STP?
9. How many liters of gaseous carbon monoxide at 27°C and 0.247atm can be produced from the burning of 65.5g of
carbon according to the following equation?
2C(s) + O2(g) → 2CO(g)
10. Air bags in cars are inflated by the sudden decomposition of sodium azide, NaN3, by the following reaction.
2NaN3(s) → 3N2(g) + 2Na(s)
What volume of N2 gas, measured at 1.30atm and 87°C, would be produced by the reaction of 70.0g of NaN3?
Unit Ten 20