Q: Which of the following is the correct equation to convert grams to moles?

$\text{Moles} = \frac{\text{Grams}}{\text{Molar Mass}}$

Q: Which of the following is the correct formula for mass/volume percent?

$\text{Mass/Volume \%} = \frac{\text{grams solute}}{\text{mL solution}} \times 100$

Question 1

Which of the following best describes Avogadro's Law?

Accepted Answer

At constant temperature and pressure, the volume of a gas is directly proportional to the number of moles of gas present. $V \propto n$

Question 2

A sample of oxygen gas occupies $12.0\ \mathrm{L}$ at $2.00\ \mathrm{atm}$ and $300\ \mathrm{K}$. What will be its volume at $1.00\ \mathrm{atm}$ and $400\ \mathrm{K}$? (Assume ideal gas behavior.)

Accepted Answer

$16.0\ \mathrm{L}$

Question 3

Which of the following is the correct equation to convert grams to moles?

Accepted Answer

$	ext{Moles} = \frac{	ext{Grams}}{	ext{Molar Mass}}$

Question 4

A barometer filled with mercury measures an atmospheric pressure of $760\ \mathrm{mmHg}$. What is this pressure in atmospheres?

Accepted Answer

$1.00\ \mathrm{atm}$

Question 5

Which solution type would cause a red blood cell to swell and possibly burst?

Accepted Answer

Hypotonic solution

Question 6

A $0.9\%$ saline solution is considered:

Accepted Answer

Isotonic to human cells

Question 7

Which of the following statements about strong electrolytes is correct?

Accepted Answer

They completely dissociate into ions in solution.

Question 8

A solution contains $10.0\ \mathrm{g}$ of NaCl dissolved in $100.0\ \mathrm{g}$ of water. What is the mass percent of NaCl in the solution?

Accepted Answer

$9.09\%$

Question 9

Which of the following best describes Dalton's Law of Partial Pressures?

Accepted Answer

The total pressure of a mixture of gases is equal to the sum of the partial pressures of each individual gas. $P_{	ext{total}} = P_1 + P_2 + \ldots$

Question 10

Which of the following is a correct application of Boyle's Law?

Accepted Answer

If the volume of a gas decreases, its pressure increases, provided temperature and amount of gas remain constant. $P_1 V_1 = P_2 V_2$

Question 11

A $2.00\ \mathrm{mol}$ sample of gas at STP occupies what volume?

Accepted Answer

$44.8\ \mathrm{L}$

Question 12

Which of the following is NOT a characteristic of a colloid?

Accepted Answer

Particles are large enough to settle out upon standing.

Question 13

Which of the following will increase the solubility of a solid solute in water?

Accepted Answer

Increasing the temperature of the solution

Question 14

A solution is prepared by dissolving $5.00\ \mathrm{g}$ of glucose ($C_6H_{12}O_6$) in enough water to make $100.0\ \mathrm{mL}$ of solution. What is the molarity of the solution? (Molar mass of glucose = $180.0\ \mathrm{g/mol}$)

Accepted Answer

$0.278\ \mathrm{M}$

Question 15

Which of the following is true about exothermic reactions?

Accepted Answer

They release heat to the surroundings.

Question 16

Which of the following is the correct formula for mass/volume percent?

Accepted Answer

$	ext{Mass/Volume \%} = \frac{	ext{grams solute}}{	ext{mL solution}} 	imes 100$

Question 17

A $250.0\ \mathrm{mL}$ solution contains $5.00\ \mathrm{g}$ of NaCl. What is the mass/volume percent of NaCl?

Accepted Answer

$2.00\%$

Question 18

Which of the following is true about suspensions?

Accepted Answer

Particles settle out upon standing.

Question 19

A $500.0\ \mathrm{mL}$ solution is diluted to $2.00\ \mathrm{L}$. If the initial concentration was $1.00\ \mathrm{M}$, what is the final concentration after dilution?

Accepted Answer

$0.25\ \mathrm{M}$

GOB Chemistry Study Notes: Moles, Gas Laws, and Solutions

Study Guide - Practice Questions

Study Guide - Flashcards