Ch 12 Gas Law Problems

0. Complete this table:

mm Hg atm. torr pascals Kilopascals bars

A.400

B. 2.5

C. 257,325

D. 1.5

1.  The air in a tank has a pressure of 640.0 mmHg at 23.0ºC. When placed in sunlight, the temperature rose to 48.0ºC. What was the pressure in the tank?

2.  A sealed glass bulb contained helium at a pressure of 92.3 kPa and a temperature of 27ºC. The bulb was packed in dry ice at -73.1ºC. What was the resulting pressure of the helium?

3.  A gas occupies a volume of 1525 mL at a temperature of 27.0ºC and 525 mmHg pressure. Calculate the volume of the gas if the temperature changed to 60.0ºC and the pressure is 725 mmHg.

4.  750.0 mL of gas at 50.2 kPa pressure and 50.0ºC is heated until the volume of gas is 2000.0 mL at a pressure of 90.0 kPa. What is the final temperature of the gas?

5.  A chemist has a certain amount of gas under a pressure of 33.3 atm; it occupies 3.0 L at 273ºC. For his research, however, the gas must be at standard conditions. Under standard conditions, what will the volume of the gas be?

6.  When J.F. Picard made a stratosphere flight in a balloon, the balloon seemed to be only half filled as it left the ground near Detroit. The gas temperature was about 27.0ºC, the pressure was 60.54 kPa, and the volume of gas in the balloon was 8000 cubic feet. What was the gas volume at high altitude where the temperature was -3ºC, and the pressure 45.5 mmHg?

7.  How many moles of hydrogen gas are present in a 5120 mL steel cylinder if the pressure is 1013.0 kPa and the temperature is 27.0ºC?

8.  How many grams of oxygen gas would occupy a 3.54 L container at 25ºC and 900.0 mmHg pressure?

9.  250 grams of nitrogen were heated to 55.0ºC in a 4500 mL container. What would be the resulting pressure?

10.  The barometric pressure on the lunar surface is about 1.0 x 10-10 mmHg. At a temperature of 100.0 K, what volume of lunar atmosphere contains 1.0 mole of molecules?

11.  A sample of exhaust gas was collected in a 1.25L tank at 752 torr. The analysis showed 92% CO2, 3.6% NO, 1.2% SO2 and 4.1% H2O. What is the partial pressure of each gas?

12.  If .05 moles of N2O4 effuse through a hole, how much NO would effuse through the same hole in the same amount of time?