Name ______
Chemistry: Gas Laws Review
P1V1 = P2V2PV = nRTPtotal = P1 + P2 + P3 . . .
V1 = V2P1V1 = P2V2
T1 T2 T1 T2
1. A pressure of 0.428 atm is exerted on a 240 ml sample of hydrogen gas. It is then increased to 0.724 atm. What will the final volume of the sample be? Show your work here!
Gas Law ______
Equation ______
Answer ______
2. A sample of air has a volume of 140.0 ml at 67°C. At what temperature will its volume be 50.0 ml? Show your work here!
Gas Law ______
Equation ______
Answer ______
3. To what new temperature must a sample of nitrogen at 27°C and 0.625 atm be taken so that its pressure becomes 1.125 atm? Show your work here!
Gas Law ______
Equation ______
Answer ______
4. A sample of gas at 47°C and 1.03 atm occupies a volume of 2.20 liters. What volume would this gas occupy at 107°C and 0.789 atm? Show your work here!
Gas Law ______
Equation ______
Answer ______
5. Three of the primary components of air are carbon dioxide, nitrogen and oxygen. In a sample containing a mixture of these gases at 760 torr of total pressure, the partial pressure of carbon dioxide is 0.285 torr and the partial pressure of nitrogen is 593.525 torr. What is the partial pressure of oxygen? Show your work here!
Gas Law ______
Equation ______
Answer ______
6. Determine the volume occupied by 0.582 mol of a gas at 15°C if the pressure is 81.8 kPa. (The gas constant R = 8.31 L·kPa/K·mol.) Show your work here!
Gas Law ______
Equation ______
Answer ______
Solve the following problems.
1. What is standard temperature and pressure?
2. What is the molar volume of all gases at STP?
3. The pressure exerted on a 240 ml sample of hydrogen gas at constant temperature is increased from 0.428 atm to 0.724 atm. What will the final volume of the sample be?
4. A sample of air has a volume of 140.0 ml at 67°C. At what temperature will its volume be 50.0 ml at constant pressure?
5. To what temperature must a sample of nitrogen at 27°C and 0.625 atm be taken so that its pressure becomes 1.125 atm at constant volume?
6. A sample of gas at 47°C and 1.03 atm occupies a volume of 2.20 L. What volume would this gas occupy at 107°C and 0.789 atm?
7. Three of the primary components of air are carbon dioxide, nitrogen, and oxygen. In a sample containing a mixture of only these gases at exactly760 torr of pressure, the partial pressures of carbon dioxide and nitrogen are given as PCO2 = 0.285 torr and PN2 = 593.525 torr. What is the partial pressure of oxygen?
8. A chemical reaction produces 0.0680 mol of oxygen gas. What volume in liters is occupied by this gas sample at STP?
9. What volume is occupied by 77.0 g of nitrogen dioxide gas at STP?
10. How many liters of oxygen gas are required to produce 30.0 liters of water, H2O?
2H2 + O2 → 2H2O
11. How many grams of aluminum oxide must be decomposed in order to produce 37.0 liters ofoxygen gas at STP?
_____Al2O3 → _____Al + _____O2
12. What volume of chlorine gas at 38°C and 1.63 atm is needed to react completely with 10.4 g of sodium to form NaCl?
Cl2 + 2Na → 2NaCl