1)Nitrogen monoxide is a pollutant commonly found in smokestack emissions. One way to remove it is to react it with ammonia.
4NH3(g) + 6NO(g) → 5N2(g) + 6H2O(ℓ)
How many liters of ammonia are required to change 17.2 L of nitrogen monoxide to nitrogen gas? Assume 100% yield and that all gases are measured at the same temperature and pressure.
L
2) What is the total volume of gaseous products formed when 38.6 liters of propane (C3H8) react completely according to the following reaction? (All gases are at the same temperature and pressure.)
Propane (C3H8)(g) + oxygen (g) → carbon dioxide(g) + water (g)
Volume = L
3) How many moles of hydrochloric acid are needed to produce 6.54 L of chlorine gas according to the following reaction at 0 °C and 1 atm?
Amount = moles
4) How many grams of calcium carbonate are needed to produce 5.20 L of carbon dioxide according to the following reaction at 25 °C and 1 atm?
calcium carbonate (s) calcium oxide (s) + carbon dioxide (g)
g calcium carbonate
5) What volume of carbon dioxide is produced when 21.3 g of calcium carbonate reacts completely according to the following reaction at 25 °C and 1 atm?
calcium carbonate (s) → calcium oxide(s) + carbon dioxide(g)
Volume = L
6) Sulfur trioxide, SO3, is produced in enormous quantities each year for use in the synthesis of sulfuric acid.
S(s) + O2(g) → SO2(g)
2SO2(g) + O2(g) → 2SO3(g)
What volume of O2(g) at 340.°С and a pressure of 5.25 atm is needed to completely convert 4.50 g sulfur to sulfur trioxide?
Volume = L
7) An important process for the production of acrylonitrile (C3H3N) is given by the following equation:
2C3H6(g) + 2NH3(g) + 3O2(g) → 2C3H3N(g) + 6H2O(g)
A 120.-L reactor is charged to the following partial pressures at 24°C:
PC3H = 0.340 MPa
PNH3 = 0.890 MPa
PO2 = 1.400 MPa
What mass of acrylonitrile can be produced from this mixture ()?
Mass = g
8) A 20.0-L nickel container was charged with 0.821 atm of xenon gas and 1.17 atm of fluorine gas at 400°C. The xenon and fluorine react to form xenon tetrafluoride. What mass (g) of xenon tetrafluoride can be produced assuming 100% yield?
g XeF4
9) Consider the unbalanced chemical equation below:
CaSiO3(s) + HF(g) → CaF2(aq) + SiF4(g) + H2O(l)
Suppose a 30.9 g sample of CaSiO3 is reacted with 32.3 L of HF at 27.0 °C and 1.00 atm. Assuming the reaction goes to completion, calculate the mass (in grams) of the SiF4 and H2O produced in the reaction.
mass SiF4 = g
mass H2O = g
10) A sample of a gas mixture contains the following quantities of three gases.
| compound | mass |
| CO | 2.46 g |
| CO2 | 1.55 g |
| SF6 | 3.90 g |
The sample has:
volume = 2.50 L
temperature = 16.6 °C
What is the partial pressure for each gas, in mmHg?
What is the total pressure in the flask?
CO mmHg
CO2 mmHg
SF6 mmHg
total mmHg
11) A mixture of xenon and helium gases is maintained in a 7.73 L flask at a pressure of 1.28 atm and a temperature of 51 °C. If the gas mixture contains 18.1 grams of xenon, the number of grams of helium in the mixture is g.
