Q: A sample of gas occupies 2.50 L at 1.00 atm and 300 K. What will be its volume at 2.00 atm and 300 K? (Assume ideal gas behavior.)

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{1.00 \times 2.50}{2.00} = 1.25\ \text{L}$$

Q: A gas sample is collected over water at 25°C. The total pressure is 760 mmHg, and the vapor pressure of water at 25°C is 24 mmHg. What is the pressure of the dry gas?

$$P_{\text{dry gas}} = 760\ \text{mmHg} - 24\ \text{mmHg} = 736\ \text{mmHg}$$

Q: A solution is prepared by dissolving 10.0 g of NaCl in 100.0 g of water. What is the mass percent of NaCl in the solution?

$$\text{Mass percent} = \frac{10.0}{10.0 + 100.0} \times 100\% = 9.09\%$$

Q: Which of the following is the correct expression for Raoult's Law?

$$P_{\text{solution}} = X_{\text{solvent}} P^0$_{\text{solvent}}$$

Question 1

Which of the following statements best explains why gases are more compressible than liquids and solids?

Accepted Answer

Gases consist of particles that are far apart with negligible volume compared to the container.

Question 2

A sample of gas occupies 2.50 L at 1.00 atm and 300 K. What will be its volume at 2.00 atm and 300 K? (Assume ideal gas behavior.)

Accepted Answer

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{1.00 	imes 2.50}{2.00} = 1.25\ 	ext{L}$$

Question 3

Which law describes the relationship between the pressure and volume of a gas at constant temperature?

Accepted Answer

Boyle's Law

Question 4

A gas sample is collected over water at 25°C. The total pressure is 760 mmHg, and the vapor pressure of water at 25°C is 24 mmHg. What is the pressure of the dry gas?

Accepted Answer

$$P_{	ext{dry gas}} = 760\ 	ext{mmHg} - 24\ 	ext{mmHg} = 736\ 	ext{mmHg}$$

Question 5

Which of the following best describes the kinetic molecular theory (KMT) of gases?

Accepted Answer

Gas particles are in constant random motion and experience elastic collisions.

Question 6

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

Accepted Answer

Hydrogen bonding

Question 7

Which of the following substances would you expect to have the highest viscosity at room temperature?

Accepted Answer

Glycerol ($$C_3H_8O_3)$$

Question 8

A solution is prepared by dissolving 10.0 g of NaCl in 100.0 g of water. What is the mass percent of NaCl in the solution?

Accepted Answer

$$	ext{Mass percent} = \frac{10.0}{10.0 + 100.0} 	imes 100\% = 9.09\%$$

Question 9

Which of the following best describes a saturated solution?

Accepted Answer

A solution in which no more solute can dissolve at a given temperature.

Question 10

Which of the following is NOT a colligative property?

Accepted Answer

Density

Question 11

A 0.10 molal aqueous solution of NaCl will have a higher boiling point than pure water. Which equation is used to calculate the boiling point elevation?

Accepted Answer

$$\Delta T_b = i K_b m$$

Question 12

Which of the following best explains why ionic compounds are generally soluble in water?

Accepted Answer

Water molecules are polar and stabilize ions through ion-dipole interactions.

Question 13

Which step in solution formation is always exothermic?

Accepted Answer

Formation of solute-solvent interactions

Question 14

A student mixes 50.0 mL of ethanol ($$C_2H_5OH) $$with 50.0 mL of water. The final volume is 97.0 mL. What type of deviation from ideal solution behavior does this represent?

Accepted Answer

Negative deviation

Question 15

Which of the following is the correct expression for Raoult's Law?

Accepted Answer

$$P_{	ext{solution}} = X_{	ext{solvent}} P^0$_{	ext{solvent}}$$

Question 16

Which of the following best describes the entropy change when a solid dissolves in water?

Accepted Answer

Entropy increases because the system becomes more disordered.

Question 17

Which of the following is true about London dispersion forces?

Accepted Answer

They arise from temporary fluctuations in electron distribution.

Question 18

A solution contains 0.50 mol of glucose ($$C_6H_{12}O_6$) dissolved in 1.0 kg of water. What is the molality of the solution?

Accepted Answer

$$m = \frac{0.50\ 	ext{mol}}{1.0\ 	ext{kg}} = 0.50\ 	ext{mol/kg}$$

Question 19

Which of the following would increase the solubility of a gas in water?

Accepted Answer

Increasing the pressure

Question 20

Which of the following is the correct order of steps in solution formation?

Accepted Answer

Breaking solute-solute interaction, breaking solvent-solvent interaction, solute-solvent interaction

Study Guide: Gases, Liquids, and Solutions (Chapters 10,11, & 13)

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