Question 1

According to the Kinetic Molecular Theory, which of the following statements best explains why gases can be compressed much more easily than solids or liquids?

Accepted Answer

Gas particles are in constant motion and have negligible volume compared to the container.

Question 2

Which of the following changes will increase the pressure of a gas in a closed, rigid container, assuming the amount of gas remains constant?

Accepted Answer

Increasing the temperature of the gas.

Question 3

A sample of gas occupies $$2.0\ \mathrm{L} at$$ $$300\ \mathrm{K}$$ and $$1.0\ \mathrm{atm}. If $$the temperature is increased to $$600\ \mathrm{K}$$ and the pressure is increased to $$2.0\ \mathrm{atm}$$, what is the new volume of the gas?

Accepted Answer

$$2.0\ \mathrm{L}$$

Question 4

Which of the following best describes what must occur for a chemical reaction to take place according to collision theory?

Accepted Answer

Particles must collide with sufficient energy and proper orientation.

Question 5

If the volume of a gas is decreased while the temperature remains constant, what happens to the pressure of the gas?

Accepted Answer

The pressure increases.

Question 6

A $$4.00\ \mathrm{L}$$ sample of gas at $$273\ \mathrm{K}$$ and $$1.00\ \mathrm{atm} is $$compressed to $$2.00\ \mathrm{L}$$ and heated to $$546\ \mathrm{K}. $$What is the new pressure?

Accepted Answer

$$4.00\ \mathrm{atm}$$

Question 7

Which of the following is NOT an assumption of the Kinetic Molecular Theory for ideal gases?

Accepted Answer

Gas particles exert attractive forces on each other.

Question 8

A rigid container holds a gas at $$2.0\ \mathrm{atm}$$ and $$300\ \mathrm{K}. If $$the temperature is doubled, what is the final pressure?

Accepted Answer

$$4.0\ \mathrm{atm}$$

Question 9

Which of the following best explains why increasing the temperature of a gas increases its pressure (in a rigid container)?

Accepted Answer

The gas particles move faster and collide with the walls more frequently and with greater force.

Question 10

A $$1.00\ \mathrm{L}$$ sample of gas at $$300\ \mathrm{K}$$ and $$1.00\ \mathrm{atm} is $$transferred to a $$2.00\ \mathrm{L}$$ container at the same temperature. What is the new pressure?

Accepted Answer

$$0.50\ \mathrm{atm}$$

Question 11

Which of the following real-life scenarios best demonstrates the relationship between gas pressure and temperature?

Accepted Answer

A car tire's pressure increases after driving on a hot day.

Question 12

Which of the following equations correctly represents the combined gas law?

Accepted Answer

$$\dfrac{P_1$ V_1$}{T_1$} = \dfrac{P_2$ V_2$}{T_2$}$$

Question 13

A $$3.00\ \mathrm{L}$$ sample of gas at $$1.00\ \mathrm{atm}$$ and $$273\ \mathrm{K} is $$changed to $$1.50\ \mathrm{L}$$ and $$546\ \mathrm{K}. $$What is the new pressure?

Accepted Answer

$$2.00\ \mathrm{atm}$$

Question 14

Which of the following would NOT increase the rate of a chemical reaction according to collision theory?

Accepted Answer

Decreasing the concentration of reactants.

Question 15

A $$2.00\ \mathrm{L}$$ sample of gas at $$300\ \mathrm{K}$$ and $$1.00\ \mathrm{atm} is $$compressed to $$1.00\ \mathrm{L} at $$constant temperature. What is the new pressure?

Accepted Answer

$$2.00\ \mathrm{atm}$$

Question 16

Which of the following best describes an elastic collision between gas particles?

Accepted Answer

No kinetic energy is lost during the collision.

Question 17

If a gas sample is cooled at constant pressure, what happens to its volume?

Accepted Answer

The volume decreases.

Question 18

Which of the following is a correct statement about the relationship between temperature and kinetic energy of gas particles?

Accepted Answer

As temperature increases, the average kinetic energy of gas particles increases.

Question 19

A $$5.00\ \mathrm{L}$$ sample of gas at $$2.00\ \mathrm{atm}$$ and $$300\ \mathrm{K} is $$changed to $$10.0\ \mathrm{L}$$ and $$600\ \mathrm{K}. $$What is the new pressure?

Accepted Answer

$$1.00\ \mathrm{atm}$$

Unit 10 Review: Gases and the Kinetic Molecular Theory

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