Question 1

A weather balloon is filled with 5.00 L of helium at 1.00 atm and 25°C. If the balloon rises to an altitude where the pressure is 0.60 atm and the temperature is -10°C, what will be the new volume of the balloon? (Assume helium behaves ideally.)

Accepted Answer

7.6 L

Question 2

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

Accepted Answer

There are fewer gas molecules per unit volume at higher altitudes.

Question 3

A scuba tank contains 12.0 L of air at a pressure of 200 atm. If the air is released into a room at 1.00 atm and 25°C, what volume will the air occupy at room conditions? (Assume temperature remains constant.)

Accepted Answer

2,400 L

Question 4

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

Accepted Answer

1 atm = 100,000 Pa

Question 5

A sample of nitrogen gas occupies 10.0 L at 27°C and 2.00 atm. How many moles of nitrogen are present? (R = 0.0821 L·atm/(mol·K))

Accepted Answer

0.81 mol

Question 6

A patient receives oxygen from a tank at 300 K and 3.00 atm. If the oxygen is delivered at 1.00 atm and 300 K, what volume of oxygen at 1.00 atm is available from 2.00 L of gas in the tank?

Accepted Answer

6.00 L

Question 7

Which scenario would most likely cause a real gas to deviate from ideal behavior?

Accepted Answer

High pressure and low temperature

Question 8

A 2.00 L flask contains 0.082 mol of argon gas at 300 K. What is the pressure inside the flask? (R = 0.0821 L·atm/(mol·K))

Accepted Answer

1.00 atm

Question 9

A gas sample is cooled from 127°C to 27°C at constant pressure. If its initial volume was 6.00 L, what is its final volume?

Accepted Answer

4.00 L

Question 10

Which of the following statements about the use of Kelvin temperature in gas law calculations is correct?

Accepted Answer

Kelvin is used because it ensures temperature values are always positive, preventing division by zero.

Question 11

A 5.00 L container holds a mixture of gases at 2.00 atm and 300 K. If the number of moles of gas is doubled while keeping temperature and volume constant, what will be the new pressure?

Accepted Answer

4.00 atm

Question 12

A barometer is used to measure atmospheric pressure. If the mercury column in a barometer falls from 760 mm Hg to 720 mm Hg, what could be a possible explanation?

Accepted Answer

A low-pressure weather system is approaching.

Question 13

A 1.00 mol sample of an ideal gas is at 1.00 atm and 273 K. What is its volume?

Accepted Answer

22.4 L

Question 14

Which of the following best describes Avogadro's Law?

Accepted Answer

At constant temperature and pressure, the volume of a gas is directly proportional to the number of moles.

Question 15

A tire is inflated to 32.0 psi at 20°C. On a hot day, the temperature rises to 40°C. Assuming the volume is constant, what is the new pressure in psi? (Use absolute temperatures.)

Accepted Answer

34.2 psi

Question 16

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

Accepted Answer

A syringe plunger is pushed in, decreasing the volume and increasing the pressure of the gas inside.

Question 17

A 10.0 L tank contains oxygen at 5.00 atm and 300 K. If 2.00 mol of oxygen are removed and the pressure drops to 3.00 atm, what is the final temperature in Kelvin? (R = 0.0821 L·atm/(mol·K))

Accepted Answer

180 K

Question 18

Which of the following is a real-world example of the combined gas law in action?

Accepted Answer

A scuba diver ascending to the surface, where both pressure and temperature change, affecting the volume of air in the lungs.

Question 19

A sample of gas at 2.00 atm and 300 K occupies 4.00 L. If the pressure is reduced to 1.00 atm and the temperature is increased to 400 K, what is the new volume?

Accepted Answer

10.7 L

Question 20

Which of the following is a common misconception about the behavior of gases?

Accepted Answer

Gases always behave ideally, regardless of pressure and temperature.

Key Concepts of Gases and Gas Laws

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