Q: A sample of nitrogen gas is at 1.00 atm in a 5.00 L container. If the volume is decreased to 2.00 L at constant temperature, what is the new pressure?

$$P_2$$ = $$P_1$$ \times \frac{$$V_1$$}{$$V_2$$} = 1.00~atm \times \frac{5.00~L}{2.00~L} = 2.50~atm$$

Q: Convert a pressure of 655 mm Hg to kilopascals ($$kPa$$). ($$1~atm = 101.3~kPa$$, $$1~atm = 760~mm~Hg)$$

$$655~mm~Hg \times \frac{101.3~kPa}{760~mm~Hg} = 87.3~kPa$$

Q: A gas is stored at 2.00 atm in a 10.0 L tank. If the gas is transferred to a 5.00 L tank at constant temperature, what is the final pressure?

$$P_2 = 2.00$$~atm \times \frac{10.0~L}{5.00~L} = 4.00~atm$$

Q: A balloon filled with helium at 1.00 atm and 2.00 L is released into the atmosphere, where the pressure drops to 0.50 atm. Assuming temperature is constant, what is the new volume of the balloon?

$$V_2$$ = $$V_1$$ \times \frac{$$P_1$$}{$$P_2$$} = 2.00~L \times \frac{1.00~atm}{0.50~atm} = 4.00~L$$

Q: A tire is inflated to 32 psi. What is the pressure in mm Hg? ($$1~atm = 14.7~psi = 760~mm~Hg)$$

$$32~psi \times \frac{760~mm~Hg}{14.7~psi} = 1,655~mm~Hg$$

Q: A gas at 1.00 atm and 3.00 L is compressed to 1.50 L at constant temperature. What is the final pressure?

$$P_2 = 1.00$$~atm \times \frac{3.00~L}{1.50~L} = 2.00~atm$$

Question 1

Which of the following best describes the shape and volume of a sample of argon gas in a closed container?

Accepted Answer

It has a variable shape and variable volume.

Question 2

A hospital stores oxygen gas at a pressure of 655 mm Hg. What is this pressure in atmospheres ($$atm$$)?

Accepted Answer

$$655 \div 760 = 0.862~atm$$

Question 3

Which change will cause the pressure of a gas in a sealed container to decrease, assuming temperature and number of molecules remain constant?

Accepted Answer

Increase the volume of the container.

Question 4

A sample of nitrogen gas is at 1.00 atm in a 5.00 L container. If the volume is decreased to 2.00 L at constant temperature, what is the new pressure?

Accepted Answer

$$P_2$$ = $$P_1$$ 	imes \frac{$$V_1$$}{$$V_2$$} = 1.00~atm 	imes \frac{5.00~L}{2.00~L} = 2.50~atm$$

Question 5

If the temperature of a gas increases while the volume and number of molecules remain constant, what happens to the pressure?

Accepted Answer

The pressure increases.

Question 6

Convert a pressure of 655 mm Hg to kilopascals ($$kPa$$). ($$1~atm = 101.3~kPa$$, $$1~atm = 760~mm~Hg)$$

Accepted Answer

$$655~mm~Hg 	imes \frac{101.3~kPa}{760~mm~Hg} = 87.3~kPa$$

Question 7

A gas is stored at 2.00 atm in a 10.0 L tank. If the gas is transferred to a 5.00 L tank at constant temperature, what is the final pressure?

Accepted Answer

$$P_2 = 2.00$$~atm 	imes \frac{10.0~L}{5.00~L} = 4.00~atm$$

Question 8

Which of the following is NOT a common unit for measuring gas pressure?

Accepted Answer

joule

Question 9

A scuba tank contains air at 3000 psi. What is this pressure in atmospheres? ($$1~atm = 14.7~psi)$$

Accepted Answer

$$3000~psi \div 14.7~psi/atm = 204~atm$$

Question 10

A balloon filled with helium at 1.00 atm and 2.00 L is released into the atmosphere, where the pressure drops to 0.50 atm. Assuming temperature is constant, what is the new volume of the balloon?

Accepted Answer

$$V_2$$ = $$V_1$$ 	imes \frac{$$P_1$$}{$$P_2$$} = 2.00~L 	imes \frac{1.00~atm}{0.50~atm} = 4.00~L$$

Question 11

Which of the following statements about gases is correct?

Accepted Answer

Gases take the shape and volume of their container.

Question 12

A tire is inflated to 32 psi. What is the pressure in mm Hg? ($$1~atm = 14.7~psi = 760~mm~Hg)$$

Accepted Answer

$$32~psi 	imes \frac{760~mm~Hg}{14.7~psi} = 1,655~mm~Hg$$

Question 13

If the number of molecules in a gas sample increases while volume and temperature remain constant, what happens to the pressure?

Accepted Answer

Pressure increases.

Question 14

A gas at 1.00 atm and 3.00 L is compressed to 1.50 L at constant temperature. What is the final pressure?

Accepted Answer

$$P_2 = 1.00$$~atm 	imes \frac{3.00~L}{1.50~L} = 2.00~atm$$

Question 15

Which of the following is a correct conversion factor for pressure units?

Accepted Answer

$$1~atm = 760~mm~Hg$$

Question 16

A gas cylinder contains 5.00 L of gas at 1.20 atm. If the gas is allowed to expand to 10.0 L at constant temperature, what is the final pressure?

Accepted Answer

$$P_2 = 1.20$$~atm 	imes \frac{5.00~L}{10.0~L} = 0.60~atm$$

Question 17

A patient receives oxygen at a pressure of 95 kPa. What is this pressure in mm Hg? ($$1~atm = 101.3~kPa = 760~mm~Hg)$$

Accepted Answer

$$95~kPa 	imes \frac{760~mm~Hg}{101.3~kPa} = 713~mm~Hg$$

Question 18

Which variable is inversely proportional to pressure for a fixed amount of gas at constant temperature?

Accepted Answer

Volume

Question 19

A gas sample at 1.50 atm is compressed from 8.00 L to 2.00 L at constant temperature. What is the final pressure?

Accepted Answer

$$P_2 = 1.50$$~atm 	imes \frac{8.00~L}{2.00~L} = 6.00~atm$$

Properties and Behavior of Gases: Pressure, Volume, and Units

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