Q: A sealed container holds a mixture of oxygen and nitrogen at 20°C. The partial pressure of oxygen is 20 kPa and nitrogen is 80 kPa. What is the total pressure in the container?

$$P_{\text{total}} = 20\,\text{kPa} + 80\,\text{kPa} = 100\,\text{kPa}$$

Q: Which of the following is the correct SI unit for pressure and its definition?

$$1\,\text{Pa} = 1\,\text{N}\,\text{m}^{-2}$$

Question 1

Which of the following statements best explains why gases are easily compressible compared to liquids and solids?

Accepted Answer

Gas particles are widely spaced and have negligible volume compared to the container.

Question 2

A sealed container holds a mixture of oxygen and nitrogen at 20°C. The partial pressure of oxygen is 20 kPa and nitrogen is 80 kPa. What is the total pressure in the container?

Accepted Answer

$$P_{	ext{total}} = 20\,	ext{kPa} + 80\,	ext{kPa} = 100\,	ext{kPa}$$

Question 3

Which property is shared by both liquids and solids but not by gases?

Accepted Answer

High density

Question 4

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

Accepted Answer

The average kinetic energy increases proportionally with temperature.

Question 5

Which of the following is the correct SI unit for pressure and its definition?

Accepted Answer

$$1\,	ext{Pa} = 1\,	ext{N}\,	ext{m}^{-2}$$

Question 6

A gas sample is cooled at constant volume. What happens to the pressure inside the container?

Accepted Answer

Pressure decreases because the average kinetic energy of particles decreases.

Question 7

Which of the following best describes the motion of gas particles according to the kinetic molecular theory?

Accepted Answer

Gas particles move rapidly in random, straight-line motion and collide elastically.

Question 8

If the volume of a gas container is doubled at constant temperature, what happens to the frequency of particle collisions with the container walls?

Accepted Answer

The frequency of collisions decreases because particles have more space to move.

Question 9

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

Accepted Answer

Gas particles have significant attractive forces between them.

Question 10

A sample of hydrogen and oxygen gases are at the same temperature. According to kinetic molecular theory, which statement is true about their average kinetic energies?

Accepted Answer

Both gases have the same average kinetic energy at the same temperature.

Question 11

Which of the following best explains why gases diffuse rapidly compared to liquids and solids?

Accepted Answer

Gas particles are widely spaced and in constant random motion.

Question 12

What is the pressure in atmospheres of a gas sample at 202.6 kPa? (Use $$1\,	ext{atm} = 101.3\,	ext{kPa})$$

Accepted Answer

$$\frac{202.6\,	ext{kPa}}{101.3\,	ext{kPa}} = 2.00\,	ext{atm}$$

Question 13

Which of the following is a real-world consequence of the non-ideal behavior of gases at high pressures?

Accepted Answer

Gases can condense into liquids due to significant intermolecular attractions.

Question 14

Which of the following best describes the relationship between pressure, force, and area?

Accepted Answer

$$P = \frac{F}{A}$$

Question 15

A gas sample at 20°C is heated to 40°C at constant volume. What happens to the pressure and why?

Accepted Answer

Pressure increases because the average kinetic energy of particles increases.

Question 16

Which of the following is the correct conversion for 760 mmHg to kPa?

Accepted Answer

$$760\,	ext{mmHg} = 101.3\,	ext{kPa}$$

Question 17

Which of the following best explains why the density of gases is much lower than that of liquids and solids?

Accepted Answer

Gas particles are widely spaced, so mass per unit volume is low.

Question 18

Which of the following is true about the kinetic energy distribution of gas particles at a given temperature?

Accepted Answer

Not all particles have the same kinetic energy; temperature reflects the average kinetic energy.

Question 19

A gas is compressed from 2.0 L to 1.0 L at constant temperature. What happens to the pressure, assuming ideal behavior?

Accepted Answer

Pressure doubles because volume is halved ($$P_1V_1 = P_2V_2).$$

Question 20

Which of the following statements about ideal and real gases is correct?

Accepted Answer

Real gases deviate from ideal behavior at low temperatures and high pressures.

Kinetic Theory of Gases and Properties of States of Matter

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