Q: Which of the following best describes Graham’s Law of Effusion?

$$\frac{\text{rate}_A}{\text{rate}_B} = \sqrt{\frac{M_B}{M_A}}$$

Question 1

A weather report states that the atmospheric pressure is 29.92 in Hg. What is this pressure in atmospheres (atm)?

Accepted Answer

$$1.00$$ atm

Question 2

According to the kinetic molecular theory, which of the following statements is TRUE for an ideal gas?

Accepted Answer

Gas particles experience negligible attractive and repulsive forces.

Question 3

A sample of gas occupies $$4.00 L at$$ $$2.00$$ atm. If the pressure is decreased to $$1.00$$ atm at constant temperature, what will be the new volume?

Accepted Answer

$$8.00 L$$

Question 4

Which equation correctly expresses Boyle’s Law?

Accepted Answer

$$P_1$$ $$V_1$$ = $$P_2$$ $$V_2$$

Question 5

A balloon filled with helium gas has a volume of $$2.50 L at$$ $$25^\circC. $$What will its volume be at $$50^\circC$$, assuming constant pressure?

Accepted Answer

$$2.72 L$$

Question 6

Which of the following best describes Avogadro’s Law?

Accepted Answer

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

Question 7

Calculate the density of $$\mathrm{O_2$}$$ gas at $$2.00$$ atm and $$273 K$$. ($$M_{O_2$} = 32.00 g/$$mol, $$R = 0.0821 L$$·atm/mol·K)

Accepted Answer

$$2.86 g/L$$

Question 8

A mixture contains $$2.0$$ mol $$\mathrm{N_2$}$$ and $$3.0$$ mol $$\mathrm{O_2$} in a$$ $$10.0 L $$container at $$300 K. $$What is the total pressure of the mixture? ($$R = 0.0821 L$$·atm/mol·K)

Accepted Answer

$$12.3$$ atm$

Question 9

Which of the following is a consequence of increasing the altitude above sea level?

Accepted Answer

Atmospheric pressure decreases because the number of gas particles per unit volume decreases.

Question 10

A $$0.500$$ mol sample of gas is confined in a $$10.0 L $$container at $$400 K. $$What is the pressure exerted by the gas? ($$R = 0.0821 L$$·atm/mol·K)

Accepted Answer

$$1.64$$ atm

Question 11

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

Accepted Answer

The volume of gas particles becomes significant compared to the container volume.

Question 12

A sample of gas has a mass of $$0.500 g$$, occupies $$0.250 L at$$ $$27^\circC $$and $$1.00$$ atm. What is the molar mass of the gas? ($$R = 0.0821 L$$·atm/mol·K)

Accepted Answer

$$65.5 g/$$mol

Question 13

Which of the following equations is used to calculate the partial pressure of a gas in a mixture?

Accepted Answer

$$P_n = X_n P_{total}$$

Question 14

Which of the following gases will effuse the fastest under identical conditions?

Accepted Answer

$$\mathrm{H_2$}$$

Question 15

A reaction produces $$0.621$$ mol of a gaseous product. If the initial volume was $$2.18 L $$with $$0.120$$ mol of gas, what is the final volume? (Assume constant $$T$$ and $$P.)$$

Accepted Answer

$$11.3 L$$

Question 16

Which of the following is the correct van der Waals equation for real gases?

Accepted Answer

$$\left( P + a \frac{n^2$}{V^2$} \right) (V - nb) = nRT$$

Question 17

Which of the following best describes Graham’s Law of Effusion?

Accepted Answer

$$\frac{	ext{rate}_A}{	ext{rate}_B} = \sqrt{\frac{M_B}{M_A}}$$

Question 18

A $$5.00 L $$container holds $$2.00$$ mol of $$\mathrm{CO_2$} at$$ $$300 K. $$What is the pressure inside the container? ($$R = 0.0821 L$$·atm/mol·K)

Accepted Answer

$$9.84$$ atm

Question 19

Which of the following is NOT a postulate of the kinetic molecular theory?

Accepted Answer

Gas particles lose energy during collisions.

Chapter 10: Gases – Properties, Laws, and Kinetic Molecular Theory

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