Q: Which of the following best describes the relationship between temperature and the root mean square velocity ($$u_{\text{rms}}) of a $$gas particle?

$$u_{\text{rms}}$$ increases as temperature increases.

Q: Which equation gives the root mean square velocity ($$u_{\text{rms}}) of a $$gas molecule?

$$u_{\text{rms}} = \sqrt{\frac{3RT}{M}}$$

Question 1

A sample of oxygen gas is collected at 25°C and 1.00 atm in a 5.00 L container. What is the mass of oxygen gas present? (Use $$R = 0.0821\ 	ext{L}\cdot	ext{atm}/	ext{mol}\cdot	ext{K}$$ and $$M_{	ext{O}_2$$} = 32.0\ 	ext{g/mol}$$)

Accepted Answer

$$6.53\ 	ext{g}$$

Question 2

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

Accepted Answer

Gas particles experience significant intermolecular forces.

Question 3

A mixture contains 2.0 mol of nitrogen and 3.0 mol of oxygen in a 10.0 L container at 300 K. What is the partial pressure of oxygen? (Use $$R = 0.0821\ 	ext{L}\cdot	ext{atm}/	ext{mol}\cdot	ext{K})$$

Accepted Answer

$$7.38\ 	ext{atm}$$

Question 4

Which of the following best describes the relationship between temperature and the root mean square velocity ($$u_{	ext{rms}}) of a $$gas particle?

Accepted Answer

$$u_{	ext{rms}}$$ increases as temperature increases.

Question 5

Which intermolecular force is primarily responsible for the high boiling point of water?

Accepted Answer

Hydrogen bonding

Question 6

A 10.0 g sample of ice at $$-10^\circ	ext{C} is $$heated to $$110^\circ	ext{C}. $$How much energy is required? (Given: $$c_{	ext{ice}} = 2.09\ 	ext{J/g}\cdot	ext{K}$$, $$c_{	ext{water}} = 4.18\ 	ext{J/g}\cdot	ext{K}$$, $$c_{	ext{steam}} = 2.01\ 	ext{J/g}\cdot	ext{K}$$, $$\Delta H_{	ext{fus}} = 334\ 	ext{J/g}$$, $$\Delta H_{	ext{vap}} = 2260\ 	ext{J/g})$$

Accepted Answer

$$7,260\ 	ext{J}$$

Question 7

Which statement about crystalline and amorphous solids is correct?

Accepted Answer

Crystalline solids have a regular, repeating structure; amorphous solids lack long-range order.

Question 8

A gas sample undergoes a change from 2.0 L at 1.0 atm to 4.0 L at constant temperature. What is the final pressure?

Accepted Answer

$$0.50\ 	ext{atm}$$

Question 9

Which equation correctly relates the density ($$d) of a $$gas to its molar mass ($$M$$), pressure ($$P$$), and temperature ($$T$$)?

Accepted Answer

$$d = \frac{PM}{RT}$$

Question 10

Which of the following best explains capillary action in water?

Accepted Answer

Strong hydrogen bonding between water molecules and the glass surface

Question 11

A 3.0 L container holds a mixture of helium and argon gases. If the mole fraction of helium is 0.60 and the total pressure is 2.0 atm, what is the partial pressure of helium?

Accepted Answer

$$1.2\ 	ext{atm}$$

Question 12

Which of the following is NOT a postulate of the kinetic molecular theory (KMT) of gases?

Accepted Answer

Gas particles exert attractive forces on each other.

Question 13

Which equation gives the root mean square velocity ($$u_{	ext{rms}}) of a $$gas molecule?

Accepted Answer

$$u_{	ext{rms}} = \sqrt{\frac{3RT}{M}}$$

Question 14

Which of the following best describes the effect of increasing atmospheric pressure on the boiling point of a liquid?

Accepted Answer

Boiling point increases as atmospheric pressure increases.

Question 15

Which intermolecular force is present in all substances, regardless of their composition?

Accepted Answer

London dispersion forces

Question 16

A balloon filled with 2.0 mol of gas at 27°C and 1.0 atm is heated to 127°C at constant pressure. What is the final volume if the initial volume was 10.0 L?

Accepted Answer

$$13.3\ 	ext{L}$$

Question 17

Which process describes the transition from solid directly to gas?

Accepted Answer

Sublimation

Question 18

Which equation represents Boyle’s Law?

Accepted Answer

$$P_1V_1 = P_2V_2$$

Question 19

Which property is most responsible for the unique behavior of water, such as its high surface tension and boiling point?

Accepted Answer

Hydrogen bonding

Question 20

Which of the following best explains why ionic compounds have higher melting points than molecular compounds?

Accepted Answer

Ionic compounds have stronger Coulombic attractions between ions.

Exam 2 Study Guide: Gases, Liquids, Solids, and Intermolecular Forces

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