Question 1

Which of the following best describes the main difference between endothermic and exothermic reactions in terms of enthalpy change ($$\Delta H$$)?

Accepted Answer

Endothermic reactions have $$\Delta H \u003e 0$$ and absorb heat from the surroundings.

Question 2

A sample of gas occupies 2.50 L at 1.00 atm and 300 K. If the pressure is increased to 2.00 atm and the temperature is decreased to 250 K, what is the new volume of the gas? (Assume ideal gas behavior.)

Accepted Answer

$$V_2 = 1.00$$\ \mathrm{L}$$

Question 3

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

Accepted Answer

Hydrogen bonding

Question 4

A solution is prepared by dissolving 10.0 g of NaCl in 100.0 g of water. Which of the following best describes the solute and solvent in this solution?

Accepted Answer

NaCl is the solute and water is the solvent.

Question 5

Which of using a catalyst in a chemical reaction is correct?

Accepted Answer

A catalyst increases the rate of reaction by providing an alternative pathway with lower activation energy.

Question 6

Given the reaction: $$2\ NO_2$(g) ightarrow 2\ NO(g) + O_2$(g)$$, if the rate law is $$	ext{Rate} = k[NO_2$]^2$$, what is the order of the reaction with respect to $$NO_2$$ and the overall order?

Accepted Answer

Second order with respect to $$NO_2$$, overall second order

Question 7

Which of the following statements about chemical equilibrium is correct?

Accepted Answer

At equilibrium, the rates of the forward and reverse reactions are equal.

Question 8

A reaction has an equilibrium constant $$K_c = 1.5 	imes 10^5$ at 25°C. What does this indicate about the reaction at equilibrium?

Accepted Answer

Products are favored at equilibrium.

Question 9

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

Accepted Answer

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

Question 10

Which equation correctly represents the relationship between pressure, volume, temperature, and number of moles for an ideal gas?

Accepted Answer

$$PV = nRT$$

Question 11

A reaction is carried out in a coffee-cup calorimeter. If the temperature of the solution increases, what can be concluded about the reaction?

Accepted Answer

The reaction is exothermic.

Question 12

Which of the following is NOT a colligative property?

Accepted Answer

Molar mass

Question 13

Which of the following best describes the effect of increasing temperature on the rate of a chemical reaction?

Accepted Answer

The rate increases because more molecules have energy greater than the activation energy.

Question 14

Which of the following is the correct expression for the equilibrium constant $$K_c$$ for the reaction: $$N_2(g) + 3H_2(g$$) \rightleftharpoons 2NH_3(g)$$?

Accepted Answer

$$K_c = \frac{[NH_3$]^2}{[N_2$][H_2$]^3}$$

Question 15

A 0.10 M solution of glucose ($$C_6H_{12}O_6$) and a 0.10 M solution of sodium chloride ($$NaCl$$) are prepared. Which solution will have the higher boiling point and why?

Accepted Answer

Sodium chloride solution, because it produces more particles in solution.

Question 16

Which of the following statements about the kinetic molecular theory of gases is FALSE?

Accepted Answer

Gas particles lose energy when they collide with each other.

Question 17

Which of the following would increase the rate of dissolution of a solid solute in a liquid solvent?

Accepted Answer

Stirring the solution

Question 18

A reaction has a rate constant $$k$$ that increases with temperature. Which equation describes this relationship?

Accepted Answer

$$k = Ae$$^{-E_a/RT}$$

Question 19

Which of the following is a real-world application of Le Chatelier’s Principle?

Accepted Answer

Increasing the pressure in the Haber process to produce more ammonia.

General Chemistry II (CH 222Z) Syllabus and Course Structure Study Guide

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