Question 1

A weather balloon is released at sea level where the atmospheric pressure is 1.00 atm and the temperature is 300 K. As it rises, the pressure drops to 0.60 atm and the temperature drops to 250 K. If the initial volume of the balloon is 2.0 L, what is its final volume? (Assume the amount of gas remains constant.)

Accepted Answer

3.6 L

Question 2

Which of the following statements best explains why atmospheric pressure decreases as altitude increases?

Accepted Answer

There are fewer gas molecules per unit volume at higher altitudes, resulting in fewer collisions with surfaces.

Question 3

A scuba diver's tank contains 12.0 L of air at a pressure of 200 atm. If the air is released at the surface where the pressure is 1.0 atm, what volume will the air occupy? (Assume constant temperature.)

Accepted Answer

2400 L

Question 4

Which of the following is NOT a correct conversion for standard atmospheric pressure?

Accepted Answer

1 atm = 1000 torr

Question 5

A gas occupies 5.0 L at 27°C and 2.0 atm. What will be its volume at 127°C and 1.0 atm? (Assume the amount of gas is constant.)

Accepted Answer

10.0 L

Question 6

A patient is administered oxygen from a tank at 3.0 atm and 10.0 L. If the oxygen is delivered at 1.0 atm, what is the maximum volume (in liters) the patient can receive at room pressure? (Assume constant temperature.)

Accepted Answer

30.0 L

Question 7

Which of the following best describes the relationship between pressure and volume for a fixed amount of gas at constant temperature?

Accepted Answer

Pressure and volume are inversely proportional.

Question 8

A 2.0 mol sample of nitrogen gas occupies 44.8 L at standard temperature and pressure (STP). If the amount of gas is doubled at constant temperature and pressure, what will be the new volume?

Accepted Answer

89.6 L

Question 9

Which of the following scenarios would most likely cause a real gas to deviate from ideal behavior?

Accepted Answer

High pressure and low temperature

Question 10

A tire is inflated to a pressure of 32 psi at 20°C. On a hot day, the temperature inside the tire rises to 50°C. Assuming the volume remains constant, what happens to the pressure inside the tire?

Accepted Answer

It increases because pressure is directly proportional to temperature in Kelvin.

Question 11

Which of the following is the correct value and units for the universal gas constant R when using the ideal gas law with pressure in atm, volume in liters, and temperature in Kelvin?

Accepted Answer

0.0821 L·atm/(mol·K)

Question 12

A sample of gas has a pressure of 500 mm Hg. What is this pressure in atmospheres?

Accepted Answer

0.658 atm

Question 13

A 1.0 L container holds 0.040 mol of helium gas at 300 K. What is the pressure inside the container? (R = 0.0821 L·atm/(mol·K))

Accepted Answer

0.984 atm

Question 14

Which of the following best explains why a barometer can be used to measure atmospheric pressure?

Accepted Answer

Atmospheric pressure pushes mercury up the tube, and the height of the mercury column reflects the pressure.

Question 15

A gas sample at 25°C and 1.0 atm is compressed from 4.0 L to 2.0 L. What is the new pressure, assuming temperature and amount of gas remain constant?

Accepted Answer

2.0 atm

Question 16

A hospital stores oxygen at 150 atm in a 50.0 L tank. How many liters of oxygen gas at 1.0 atm can be supplied to patients at room temperature?

Accepted Answer

7500 L

Question 17

Which of the following is a correct application of Avogadro's Law?

Accepted Answer

Doubling the number of moles of gas at constant temperature and pressure doubles the volume.

Question 18

A gas is collected over water at 25°C and a total pressure of 755 mm Hg. The vapor pressure of water at 25°C is 23.8 mm Hg. What is the partial pressure of the gas collected?

Accepted Answer

731.2 mm Hg

Question 19

Which of the following best describes why real gases deviate from ideal behavior at high pressures?

Accepted Answer

At high pressures, gas molecules are closer together and intermolecular forces become significant.

Key Concepts of Gases and Gas Laws

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