#
Name:
Date:
Worksheet: Ideal Gas Law Equation, Combined Gas Law Equation, and Manipulations
Mixed Practice—you will first need to determine which formula to use and then solve the problem. Think about the
context of each set up.
1. In a thermonuclear device (i.e., nuclear bomb), the pressure of 0.050 liters of gas within the bomb casing reaches 4.0 x
106 atm. When the bomb casing is destroyed by the explosion, the gas is released into a specially designed testing room
where it reaches a pressure of 1.00 atm. What is the volume of the gas after the explosion?
2. Determine the molar mass of a gas that has a density of 2.18 g/L at 66°C and 720 mm Hg.
3. Synthetic diamonds can be manufactured at pressures of 6.00 x 104 atm. If we took 2.00 liters of gas at 1.00 atm and
compressed it to a pressure of 6.00 x 104 atm, what would the volume of that gas be?
4. A sample of nitrogen gas, N2, is collected in a100 mL container at a pressure of 688 mm Hg and a temperature of
565 °C. How many grams of nitrogen gas are present in this sample?
5. How many moles of chlorine gas would occupy a volume of 35.5 L at a pressure of 100.0 kPa and a temperature of
100. C? After determining the number of moles, calculate the number of grams of chlorine (Cl2) contained in this
container?
6. Use the following reaction to answer the next few questions: 2 C8H18(l) + 25O2(g)  16CO2(g) + 18H2O(g) The above
reaction is the reaction between gasoline (octane) and oxygen that occurs inside automobile engines.
A. If 4.00 moles of gasoline are burned, what volume of oxygen is needed if the pressure is 0.953 atm, and the
temperature is 35.0°C?
B. How many grams of water would be produced if 20.0 liters of oxygen were burned at a temperature of -10.0°C
and a pressure of 1.3 atm?
7. Determine the density of hydrogen bromide gas at 3.10 atm and -5°C.
8. A series of measurements are made in order to determine the molar mass of an unknown gas. First, a large flask is
evacuated and found to weigh 134.57g. It is then filled with the gas to a pressure of 735 torr at 31°C. It is reweighed
and its mass is now 137.456g. Finally, the flask is filled with water at 31°C and found to weigh 1067.9g. (The density
of water at this temperature is 0.998 g/mL.) Assuming the ideal-gas equation applies, calculate the molar mass of the
unknown gas.
9. CaCO3 decomposes at 1200ºC to form CO2 gas and CaO. If 25 L of CO2 are collected at 12000 C and 25 atm, how
many grams of CaCO3 must have decomposed?