Q: Graham's Law of Effusion can be derived from which of the following relationships?

$$ \frac{\text{Rate}_1}{\text{Rate}_2} = \sqrt{\frac{M_2$}{M_1$}} $$

Question 1

According to the Kinetic Molecular Theory, which of the following statements is NOT an assumption made about ideal gases?

Accepted Answer

Gas particles experience significant attractive and repulsive forces.

Question 2

Which equation correctly relates the average kinetic energy of a gas particle to temperature?

Accepted Answer

$$ KE = \frac{3}{2} k_B T $$

Question 3

A balloon filled with helium is released on a cold day. According to the Kinetic Molecular Theory, what happens to the average kinetic energy of the helium atoms as the temperature decreases?

Accepted Answer

The average kinetic energy decreases.

Question 4

Which of the following best explains why lighter gas molecules move faster than heavier ones at the same temperature?

Accepted Answer

Lighter molecules have the same kinetic energy but lower mass, resulting in higher velocity.

Question 5

Graham's Law of Effusion can be derived from which of the following relationships?

Accepted Answer

$$ \frac{	ext{Rate}_1}{	ext{Rate}_2} = \sqrt{\frac{M_2$}{M_1$}} $$

Question 6

If the temperature of a gas is doubled, what happens to the root mean square speed ($$v_{rms}) of $$its molecules?

Accepted Answer

$$ v_{rms} $$ increases by a factor of $$ \sqrt{2} $$

Question 7

A sample contains equal moles of $$ \mathrm{H_2$} $$ and $$ \mathrm{O_2$}  at $$the same temperature. Which statement is true about their average velocities?

Accepted Answer

$$ \mathrm{H_2$} $$ molecules move faster than $$ \mathrm{O_2$} $$ molecules.

Question 8

Which real-world scenario best illustrates Graham's Law of Effusion?

Accepted Answer

Helium escapes from a balloon faster than oxygen.

Question 9

If the molar mass of gas A is 4 g/mol and gas B is 36 g/mol, what is the ratio of their rates of effusion ($$ \frac{	ext{Rate}_A}{	ext{Rate}_B} $$)?

Accepted Answer

$$ 3 $$

Question 10

Which of the following changes would cause the pressure inside a rigid container of gas to decrease, according to the Kinetic Molecular Theory?

Accepted Answer

Decreasing the temperature of the gas.

Question 11

A rigid tank contains nitrogen gas at 300 K. If the temperature is increased to 600 K, what happens to the average kinetic energy of the nitrogen molecules?

Accepted Answer

It doubles.

Question 12

Which of the following is a direct consequence of the assumption that gas particles are in constant, random motion?

Accepted Answer

Gases fill their containers uniformly.

Question 13

A gas sample is cooled at constant volume. Which of the following best describes what happens to the frequency and force of collisions with the container walls?

Accepted Answer

Both frequency and force of collisions decrease.

Question 14

Which formula gives the root mean square speed ($$v_{rms}) of a $$gas molecule?

Accepted Answer

$$ v_{rms} = \sqrt{\frac{3RT}{M}} $$

Question 15

Which of the following best explains why a balloon shrinks when placed in a freezer?

Accepted Answer

The kinetic energy of the gas particles decreases, leading to lower pressure inside the balloon.

Kinetic Molecular Theory and Graham's Law of Effusion

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