Q: A sample of gas at 2.00 atm is compressed from 4.00 L to 2.00 L at constant temperature. What is the new pressure?

$P_1V_1 = P_2V_2$; $P_2 = \frac{P_1V_1}{V_2} = \frac{2.00 \times 4.00}{2.00} = 4.00$ atm

Question 1

Which of the following statements best describes the Kinetic Molecular Theory as it applies to gases?

Accepted Answer

Gas particles are in constant, random motion and collisions between them are perfectly elastic.

Question 2

Which of the following is NOT a factor that affects gas pressure according to the ideal gas law?

Accepted Answer

Type of gas (identity of the molecule)

Question 3

A sample of gas at 2.00 atm is compressed from 4.00 L to 2.00 L at constant temperature. What is the new pressure?

Accepted Answer

$P_1V_1 = P_2V_2$; $P_2 = \frac{P_1V_1}{V_2} = \frac{2.00 	imes 4.00}{2.00} = 4.00$ atm

Question 4

Which equation correctly relates pressure, volume, temperature, and moles for an ideal gas?

Accepted Answer

$PV = nRT$

Question 5

If the temperature of a gas is doubled while keeping the volume and number of moles constant, what happens to the pressure?

Accepted Answer

The pressure is doubled.

Question 6

Which of the following best describes the process of hydration when a solute dissolves in water?

Accepted Answer

Water molecules surround and interact with solute ions or molecules via dipole interactions.

Question 7

Which statement correctly defines a saturated solution?

Accepted Answer

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

Question 8

Which of the following substances is most likely to be a strong electrolyte in water?

Accepted Answer

Sodium chloride ($NaCl$)

Question 9

A student mixes 0.50 mol of $Na_2SO_4$ with 1.00 mol of $BaCl_2$ in water. What is the limiting reactant in the reaction $BaCl_2 + Na_2SO_4 \rightarrow BaSO_4 + 2NaCl$?

Accepted Answer

$Na_2SO_4$ is the limiting reactant.

Question 10

Which of the following best describes Le Chatelier's Principle?

Accepted Answer

A system at equilibrium will shift to counteract any imposed change in concentration, temperature, or pressure.

Question 11

Which of the following is the correct expression for the equilibrium constant $K_c$ for the reaction $2NO_2 \rightleftharpoons N_2O_4$?

Accepted Answer

$K_c = \frac{[N_2O_4]}{[NO_2]^2}$

Question 12

If $K_c$ for a reaction is much greater than 1, what does this indicate about the equilibrium mixture?

Accepted Answer

The mixture contains mostly products.

Question 13

Which of the following is a correct application of the mole-to-mole ratio in a chemical reaction?

Accepted Answer

Using the coefficients in a balanced equation to convert between moles of reactants and products.

Question 14

Which of the following is true about weak electrolytes?

Accepted Answer

They partially dissociate into ions in solution.

Question 15

A solution is prepared by dissolving 0.10 mol of $KCl$ in enough water to make 1.0 L of solution. What is the molarity of the solution?

Accepted Answer

$M = \frac{0.10}{1.0} = 0.10$ M

Question 16

Which of the following is the correct formula for converting pressure from atm to mmHg?

Accepted Answer

$P_{mmHg} = P_{atm} 	imes 760$

Question 17

Which of the following best describes the role of $K_{sp}$ in chemistry?

Accepted Answer

It is the equilibrium constant for the solubility of a sparingly soluble salt.

Question 18

A chemical reaction is at equilibrium. If more reactant is added, what will happen according to Le Chatelier's Principle?

Accepted Answer

The equilibrium will shift to produce more products.

Question 19

Which of the following is a correct statement about the effect of temperature on the solubility of most solid solutes in water?

Accepted Answer

Solubility increases as temperature increases.

Question 20

Which of the following is the correct formula for calculating the concentration of a solution after dilution?

Accepted Answer

$M_1V_1 = M_2V_2$

General Chemistry Study Guide: Gases, Solutions, and Chemical Equilibrium

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