CH 11 Honors Chemistry Gas Laws
1. An aerosol can contain 400. mL of compressed gas at 5.20 atm pressure. When all the gas is
sprayed into a large plastic bag, the bag inflates to a volume of 2.14L. What is the pressure
inside the plastic bag? Assume temperature is constant. [0.972 atm]
2. If 0.500 mol of nitrogen gas occupies a volume of 11.2 L at 0C, what volume will 2.00 mol of
nitrogen gas occupy at the same temperature & pressure? [44.8 L]
3. Given the following 2 NO2(g)  N2O4(g) If 25.0 mL of NO2 gas is completely converted to N2O4
gas at STP, what volume will the N2O4 gas occupy? [12.5 mL]
4. A steel reaction vessel of a bomb calorimeter, which has a volume of 750 mL, is charged with
oxygen gas to a pressure of 145 atm at 22.0C. Calculate the mass of oxygen in the reaction
vessel. [143.7 g]
5. A particular balloon is designed by its manufacturers to be inflated to a volume no more than
2.5 L. If the balloon is filled with 2.0 L of helium at sea level, is released and rises to an altitude
at which the atmospheric pressure is only 500.0 mmHg, will the balloon burst. Temperature is
constant. [3.04 L will burst]
6. What mass of He is required to fill a 1.5 L balloon at STP? [0.268 g]
7. A student adds 4.00g of dry ice (solid CO2) to an empty balloon. What will be the volume the
balloon at STP after all the dry ice sublimes? [2.04 L]
8. What volume (mL) of oxygen gas, measured at 30.0C and 725 torr, can be produced from the
complete decomposition of 4.10 g of mercuric oxide? [247.7 mL]
9. Given the following reaction CO + 2H2  CH3OH. Hydrogen at STP flows into a reactor at a rate
of 16.0 L/min and carbon monoxide at STP flows into the reactor at a rate of 25.0 L/min. If 5.30 g
of CH3OH is produced per min, what is the percent yield of the reaction? [46.5 %]
10. A mixture of 1.00 g H2 and 1.00 g of He is placed in a 1.00 L container at 27.0C. Calculate the
partial pressure of each gas and the total pressure (mmHg). [9360 mmHg H2, 4680 mmHg He,
14040 mmHg total]
11. A compound contains only nitrogen and hydrogen and is 87.4% nitrogen by mass. A gaseous
sample of this compound has a density of 0.977 g/L at 710 torr and 100.0C. What is the
molecular formula of this compound? [N2H4]
12. Uranium hexafluoride is solid at room temperature, but it boils at 56.0C. Determine the density
of uranium hexafluoride at 60.0C and 745 torr. [12.6 g/L]
13. A chemist weighs out 5.14g of a mixture containing unknown amounts of BaO and CaO and
placed the sample in a 1.50L flask containing CO2 at 30.0C and 750 torr. After the reaction to
form BaCO3 and CaCO3 was completed, the pressure of CO2 remaining was 230 torr. Calculate
the mass percentages of CaO and BaO in the mixture and the moles of CO2 in excess. [88.7 %
BaO, 11.3% CaO]
14. At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen
gas. A 0.8765g sample of impure sodium chlorate was heated until the production of oxygen
ceased. The oxygen collected over water occupied 57.2 mL at a temperature of 22.0 C and a
pressure of 734 mmHg. Calculate the mass percent of NaClO3 in the original sample. (Vapor
pressure of water at 22.0 C is 19.8 mmHg) [17.5%]
15. Calculate the density of ammonia gas at 27.0C and 635 torr. [0.611 g/L]
16. A compound has the empirical formula CHCl. A 256 mL flask at 373 K and 750 mmHg contains
0.800g of the gaseous compound. Find the molecular formula. [C2H2Cl2]
17. At 0C a 1.0 L flask contains 5.0 x10-2 moles of N2, 1.5 x102 mg O2 and 5.0 x1021 molecules of NH3.
What is the partial pressure of each gas and what is the total pressure in the flask. [851.8 mmHg
N2, 79.9 mmHg O2, 141.4 mmHg NH3, 1073.1 mmHg Total]
18. A 2.00 L sample of O2 was collected over water at a total pressure of 104.66 kPa and 25C. When
the O2 was dried, the gas had a volume of 1.94 L at 25 C and 785 torr. Calculate the vapor
pressure of water at 25 C. [24.0 torr]
19. A gas consisting of only carbon and hydrogen has an empirical formula of CH2. The gas has a
density of 1.65 g/L at 27C and 0.966 atm. Determine the molar mass and the molecular formula
of the gas. [42.1 g/n, C3H6]
20. Given the balanced equation, 2C3H6 g + 2NH3 g + 3O2 g 2C3H3N g + 6H2O g, if you have 250 mL
of C3H6 and 500 mL of oxygen at 744.0 mmHg and 25.0C with excess NH3, calculate the moles of
water produced, the excess volume (mL)of the other reactant that you were given information
about and the moles of H atoms in the water produced. If 0.25g of water was produced,
calculate the percent yield. [0.03n H2O, 125.1 mL excess, 0.06n H, 46.3% yield]