Question 1

Which of the following best describes the motion of gas particles as shown in the first image?

Accepted Answer

Gas particles move in straight lines until they collide with each other or the container walls.

Question 2

According to the kinetic molecular theory, what happens to the average kinetic energy of gas particles when the temperature increases?

Accepted Answer

It increases.

Question 3

Refer to the second image. What law is being demonstrated by the relationship between pressure and volume in the two containers?

Accepted Answer

Boyle's Law

Question 4

Which equation correctly represents Boyle’s Law as shown in the images?

Accepted Answer

$$P_1V_1 = P_2V_2$$

Question 5

A gas occupies a volume of 2.0 L at a pressure of 100 kPa. If the pressure is increased to 200 kPa at constant temperature, what will the new volume be?

Accepted Answer

1.0 L

Question 6

Which graph (see third image) best represents the relationship between pressure and volume for a fixed amount of gas at constant temperature?

Accepted Answer

A curve that decreases as volume increases

Question 7

What is the significance of the dashed line in the fifth image, which shows a deviation from the expected pressure-volume curve?

Accepted Answer

It shows the deviation of a real gas from ideal behavior at high pressure.

Question 8

Which of the following is NOT an assumption of the kinetic molecular theory for ideal gases?

Accepted Answer

Gas particles lose energy during collisions.

Question 9

A weather balloon is released at 25°C (298 K), with a volume of 12.6 m³ and a pressure of 105,000 Pa. When it bursts, the pressure is 27,640 Pa and the volume is 36.3 m³. Using the combined gas law, what is the temperature (in Kelvin) when it bursts? (Use $$\frac{P_1V_1}{T_1$} = \frac{P_2V_2}{T_2$})$$

Accepted Answer

240 K

Question 10

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

Accepted Answer

The volume of gas particles and intermolecular forces become significant.

Question 11

Which equation would you use to calculate the number of moles of a gas if you know its pressure, volume, and temperature?

Accepted Answer

$$PV = nRT$$

Question 12

A 0.5 m³ container holds 2 mol of gas at a temperature of 300 K. What is the pressure inside the container? (Use $$R = 8.31 J$$·K⁻¹·mol⁻¹ and $$PV = nRT)$$

Accepted Answer

9,972 N/m²

Question 13

Which of the following statements about the ideal gas law is correct?

Accepted Answer

It is most accurate for gases at high temperature and low pressure.

Question 14

A gas sample has a mass of 0.77 g, occupies a volume of 0.32 dm³ at 27°C and a pressure of 96 kPa. What is the molar mass of the gas? (Use $$PV = nRT$$, $$R = 8.31 J$$·K⁻¹·mol⁻¹, and $$T in $$Kelvin)

Accepted Answer

20 g/mol

Question 15

Which of the following is a real-life example of Charles’s Law?

Accepted Answer

A balloon shrinks when placed in a freezer.

Question 16

Which variable must remain constant when using Boyle’s Law to solve a problem?

Accepted Answer

Temperature

Question 17

If a car tire is inflated to a certain pressure at 20°C and then driven until the air inside reaches 50°C, what happens to the pressure inside the tire (assuming volume is constant)?

Accepted Answer

It increases.

Question 18

Which of the following is the correct conversion from Celsius to Kelvin?

Accepted Answer

$$K = ^\circ C + 273$$

Gas Laws and the Behavior of Gases: Study Notes for Introductory Chemistry

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