Q: A mixture contains 2.0 mol $$N_2$$ and 3.0 mol $$O_2 in a 10.0 L $$container at 300 K. What is the partial pressure of $$O_2$$? ($$R = 0.0821\ \text{L·atm·mol}^{-1}\text{K}^{-1})$$

$$P_{O_2$} = 4.92\ \text{atm}$$

Q: A solution is made by dissolving 0.50 mol of glucose (a non-volatile solute) in 1.00 kg of water. If the vapor pressure of pure water at this temperature is 23.8 mmHg, what is the vapor pressure of the solution? (Assume ideal behavior.)

$$P_{\text{soln}} = 21.2\ \text{mmHg}$$

Question 1

A sample of nitrogen gas occupies 5.00 L at 27°C and 2.00 atm. If the gas is compressed to 3.00 L and heated to 77°C, what is the final pressure of the gas? (Assume ideal behavior.)

Accepted Answer

$$P_2 = 3.85$$\ 	ext{atm}$$

Question 2

Which of the following gases will have the highest root mean square speed ($$\mu_{	ext{rms}}) at 298 K$$?

Accepted Answer

Helium (He)

Question 3

A 2.00 g sample of an unknown gas occupies 1.50 L at 1.00 atm and 25°C. What is the molar mass of the gas?

Accepted Answer

$$M = 32.6\ 	ext{g/mol}$$

Question 4

Which intermolecular force is primarily responsible for the high boiling point of water compared to other group 16 hydrides?

Accepted Answer

Hydrogen bonding

Question 5

Which of the following statements about real gases is correct?

Accepted Answer

Real gases deviate from ideal behavior due to intermolecular forces and finite molecular volume.

Question 6

A mixture contains 2.0 mol $$N_2$$ and 3.0 mol $$O_2 in a 10.0 L $$container at 300 K. What is the partial pressure of $$O_2$$? ($$R = 0.0821\ 	ext{L·atm·mol}^{-1}	ext{K}^{-1})$$

Accepted Answer

$$P_{O_2$} = 4.92\ 	ext{atm}$$

Question 7

Which of the following molecules is nonpolar, despite having polar bonds?

Accepted Answer

Carbon dioxide ($$CO_2)$$

Question 8

Which of the following best explains why iodine ($$I_2) is a $$solid at room temperature while chlorine ($$Cl_2) is a $$gas?

Accepted Answer

Iodine has stronger dispersion forces due to its larger size.

Question 9

A solution is made by dissolving 0.50 mol of glucose (a non-volatile solute) in 1.00 kg of water. If the vapor pressure of pure water at this temperature is 23.8 mmHg, what is the vapor pressure of the solution? (Assume ideal behavior.)

Accepted Answer

$$P_{	ext{soln}} = 21.2\ 	ext{mmHg}$$

Question 10

Which of the following substances can form hydrogen bonds?

Accepted Answer

Hydrogen fluoride ($$HF)$$

Question 11

Which property of water decreases as it is cooled from 4°C to 0°C?

Accepted Answer

Density

Question 12

Which of the following best describes the effect of increasing temperature on the vapor pressure of a liquid?

Accepted Answer

Vapor pressure increases exponentially.

Question 13

A solution is prepared by dissolving 0.10 mol NaCl in 1.00 kg of water. What is the van’t Hoff factor ($$i) $$for NaCl in this solution, assuming complete dissociation?

Accepted Answer

$$i = 2$$

Question 14

Which of the following statements about colligative properties is correct?

Accepted Answer

They depend only on the number of solute particles.

Question 15

Which of the following best describes the process of effusion?

Accepted Answer

The escape of gas molecules through a small hole into a vacuum.

Question 16

Which of the following molecules has the highest boiling point?

Accepted Answer

Ammonia ($$NH_3)$$

Question 17

A 0.20 m aqueous solution of a non-electrolyte has a freezing point depression constant $$K_f = 1.86\ ^\circ	ext{C·kg·mol}^{-1}. $$What is the expected freezing point of the solution?

Accepted Answer

$$-0.37\ ^\circ	ext{C}$$

Question 18

Which of the following best explains why salt is spread on icy roads in winter?

Accepted Answer

Salt lowers the freezing point of water, causing ice to melt.

Question 19

Which of the following is the correct expression for the density of a gas using the ideal gas law?

Accepted Answer

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

Question 20

Which of the following best describes the relationship between intermolecular forces and viscosity?

Accepted Answer

Stronger intermolecular forces lead to higher viscosity.

General Chemistry Study Guide: Gases, Intermolecular Forces, and Solutions

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