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2. At standard temperature and a pressure of 619 kPa, a sample of Cl₂ gas has a volume of 31.2 liters. How many grams of gas are in the sample?â g

1. Find the volume of 6.50 mol of an ideal gas at 24.0Â°C and a pressure of 419 kPa. Use the ideal gas law and

R = 0.0821 atm â¢ L/mol â¢ K. ___________L

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Two parts

(A) A 2.38 L sample of gas is warmed from 250.0 K to a final temperature of 472.0 K. Assuming no change in pressure, what is the final volume of the gas?

(B) Find the volume in milliliters of 2.00 mol of an ideal gas at 35Â°C and a pressure of 1110 torr.

Use the ideal gas law and the appropriate R value:

R = 0.0821 atm â¢ L/mol â¢ K

R = 8.31 kPa â¢ L/mol â¢ K

R = 62.4 torr â¢ L/mol â¢ K

Use the ideal gas law to calculate the volume occupied by 0.300 mol of nitrogen gas at 1.40 atm pressure and at 27Â°C. R = 0.0821 L * atm/(K*mol).

Applying Ideal Gas Laws Problems

Name: ________________________

1. A sample of hydrogen gas at a temperature of 40 K changes its volume from 50 liters to 30 liters. What is the new temperature after the reduction in volume?

2. A sample of radon gas at 300 kPa and 120 ⁰C, and cools down to 80 ⁰C. What is the new pressure if the number of moles and volume remains the same?

3. A sample of nitrogen gas has a pressure of 2.50 atm at a temperature of 25⁰C. What temperature is required to increase the pressure to 4.00 atm, assuming the volume is fixed and the amount of gas does not change?

4. What happens to the pressure inside a rigid container if the amount of nitrogen gas increases from 0.500 mole to 0.750 mole? The original pressure is 98.0 kPa, and the temperature remains constant.

5. The volume of a sample of gas is 200 mL at 275 K and 0.891 atm. What will the new volume of the gas be at 77⁰C and 98.5 kPa?

6. What is the volume occupied by 36.0 grams of water vapor at a temperature of 125⁰C and a pressure of 102 kPa?

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