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

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

Q: A solution is prepared by dissolving 10.0 g of NaCl in enough water to make 500 mL of solution. What is the molarity of the solution? ($$\mathrm{NaCl}$$ molar mass = $$58.44\ \mathrm{g/mol})$$

$$M = \frac{10.0\ \mathrm{g}}{58.44\ \mathrm{g/mol} \times 0.500\ \mathrm{L}} = 0.342\ \mathrm{M}$$

Question 1

Which of the following is NOT an assumption of the kinetic molecular theory for ideal gases?

Accepted Answer

Gas particles experience significant attractive and repulsive forces.

Question 2

A sample of nitrogen gas occupies 2.50 L at 1.00 atm and 300 K. What will be its volume at 2.00 atm and 300 K, assuming ideal gas behavior?

Accepted Answer

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

Question 3

Which of the following correctly describes the relationship between temperature and kinetic energy for gases?

Accepted Answer

As temperature increases, the average kinetic energy of gas particles increases.

Question 4

Which equation is used to relate pressure, volume, temperature, and moles for an ideal gas?

Accepted Answer

$$PV = nRT$$

Question 5

A solution is prepared by dissolving 10.0 g of NaCl in enough water to make 500 mL of solution. What is the molarity of the solution? ($$\mathrm{NaCl}$$ molar mass = $$58.44\ \mathrm{g/mol})$$

Accepted Answer

$$M = \frac{10.0\ \mathrm{g}}{58.44\ \mathrm{g/mol} 	imes 0.500\ \mathrm{L}} = 0.342\ \mathrm{M}$$

Question 6

Which statement best describes a saturated solution?

Accepted Answer

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

Question 7

Which of the following will increase the boiling point of water?

Accepted Answer

Adding NaCl to the water.

Question 8

Which formula is used to calculate the number of moles of solute in a solution given its molarity and volume?

Accepted Answer

$$n = M 	imes V$$

Question 9

Which of the following is a property of acids?

Accepted Answer

They turn blue litmus paper red.

Question 10

A solution has a pH of 3. Which of the following best describes this solution?

Accepted Answer

It is acidic.

Question 11

Which of the following is the correct formula for calculating the pH of a solution from its hydrogen ion concentration?

Accepted Answer

$$\mathrm{pH} = -\log[\mathrm{H}^+]$$

Question 12

Which of the following best describes a buffer solution?

Accepted Answer

A solution that resists changes in pH when small amounts of acid or base are added.

Question 13

Which of the following is true about the periodic trend in atomic radius across a period?

Accepted Answer

Atomic radius decreases from left to right across a period.

Question 14

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

The azimuthal quantum number ($$l)$$

Question 15

Which of the following elements has the highest first ionization energy?

Accepted Answer

Neon (Ne)

Question 16

Which statement best explains why atomic radius increases down a group in the periodic table?

Accepted Answer

Additional electron shells are added, increasing the distance from the nucleus.

Question 17

Which of the following is the correct electron configuration for a neutral oxygen atom?

Accepted Answer

$$1s^2$$\ $$2s^2$$\ $$2p^4$$

Question 18

A student mixes 100 mL of 0.50 M HCl with 100 mL of 0.50 M NaOH. What is the pH of the resulting solution?

Accepted Answer

The solution is neutral; $$\mathrm{pH} = 7$$

Question 19

Which of the following best describes the difference between a strong acid and a weak acid?

Accepted Answer

A strong acid completely ionizes in water, while a weak acid only partially ionizes.

General Chemistry Study Guide: Gases, Solutions, Acids & Bases, and Atomic Structure

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