Gas Law Problems WS
These are “1” problems: Basic understanding
1. Calculate the volume in liters occupied by 0.55 kg of dimethyl ether, C2H6O, at 950mmHg and 15C.
2. The ozone molecules in the atmosphere absorb much of the ultraviolet radiation from the sun. The
temperature of the stratosphere is -23C and the pressure due to the ozone is 1.4 x 10-7 atm. Calculate
the number of ozone molecules present in 1.0ml.
3. Calculate the density of the gas, CF2Cl2, at 0C and 1.00atm.
4. Butane, C4H10, is an easily liquefied gaseous fuel. Calculate the density of butane gas at 1.00atm and
25C. Give your answer in grams per liter.
These are “3” problems: Application of knowledge
5. Acetylene is prepared by the reaction of calcium carbide with water:
CaC2(s) + 2H2O(l)
Ca(OH)2(s) + C2H2(g)
What volume of acetylene can be obtained from 100 grams of calcium carbide and 100 grams of water
at 0C and 1.00atm? What volume results when the temperature is 120C and the pressure is 1.00atm?
6. Cellular respiration occurs according to the overall equation:
C6H12O6(s) + 6O2(g)
6CO2(g) + 6H2O(g)
Calculate the volume of CO2 produced at 37C and 1.00atm when 1.00 gram of glucose is metabolized.
7. A 1.28 gram sample of a colorless liquid was vaporized in a 250ml flask at 121C and 786mmHg. What is
the molecular weight of this substance?
8. Chlorine is produced by the electrolysis of an aqueous solution:
2NaCl(aq) +2H2O(l)
2NaOH(aq) + H2(g) + Cl2(g)
The hydrogen gas and chlorine gas are collected separately at 10.0atm and 25C. What volume of each
gas can be obtained from 2.50kg of NaCl?
9. A 0.271 gram sample of an unknown vapor occupies 249ml 1t 100C and 765mmHg. The simplest
formula of the compound is CH2. What is the molecular formula of the compound?
10. Upon chemical analysis, a gaseous hydrocarbon is found to contain 88.82% carbon and 11.18%
hydrogen by mass. A 62.6 gram sample of the gas occupies 34.9ml at 772mmHg and 100C. Determine
the molecular formula of the compound?
11. A gaseous mixture consists of 0.513 grams of H2 and 16.1 grams of N2 occupies 10.0L at 20C. Calculate
the partial pressure of H2 and N2 in the mixture.
12. When carbon dioxide is bubbled into a solution of calcium hydroxide, Ca(OH)2, calcium carbonate
precipitates: Ca(OH)2(aq) + CO2(g)
CaCO3(s) + H2O(l)
During a particular experiment, 2.35 grams of calcium carbonate were formed. How many liters of
carbon dioxide at 15C and 775mmHg must have been bubbled into a solution of calcium hydroxide to
give this quantity of calcium carbonate?
13. In the Solvay process, ammonia and carbon dioxide are passed into a solution of sodium chloride.
Sodium hydrogen carbonate, NaHCO3, precipitates from the solution.
NH3(g) + CO2(g) + H2O(g) + NaCl(s)
NaHCO3(s) + NH4Cl(aq)
How many liters of ammonia at 5C and 2.00atm are required to produce 1.00kg of NaHCO3?
These are “5” problems: Synthesis and evaluation
14. Nitroglycerin decomposes according to the equation:
4C3H5(NO3)3(s)
12CO2(g) + 10H2O(l) + 6N2(g) + O2(g)
What is the total volume of gases produced when collected at 1.0atm and 25C from 10.0 grams of
nitroglycerin? What pressure is produced if the reaction is confined to a volume of 0.50L at 25C?
Assume that you can use the ideal gas equation. Neglect any pressure due to water vapor.
15. Lithium metal reacts with nitrogen at room temperature, 20C, according to the equation:
6Li(s) + N2(g)
2Li3N2(s)
A sample of lithium metal was placed under a nitrogen atmosphere in a sealed 1.00L container at a
pressure of 1.23 atm. One hour later the pressure dropped to 0.92atm. Calculate the number of grams
of nitrogen that reacted with the lithium metal. Assuming that all the lithium metal reacted, calculate
the mass of lithium originally present.
16. A 0.2036 gram sample of an unknown compound, consisting of C, H, O and N, is combusted in excess
oxygen. From this reaction, 0.122grams of H2O(l) and 132.9ml of CO2(g) are recovered at a temperature
of 298K and 1.00atm. In a separate experiment, 0.2500grams of the unknown compound results in the
formation of 40.0ml of nitrogen gas at 25C and 1.00atm. Determine the empirical formula of this
unknown compound.