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?
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.
