Question 1

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

Accepted Answer

If a system at equilibrium is disturbed, the system will shift to minimize the disturbance and reestablish equilibrium.

Question 2

Consider the equilibrium: $$\mathrm{N_2O_4(g) \rightleftharpoons 2 NO_2$(g)}. At $$equilibrium, $$[NO_2$] = 5\ \mathrm{M}$$ and $$[N_2O_4] = 4\ \mathrm{M}. If $$more $$NO_2 is $$added and equilibrium is reestablished at $$[NO_2$] = 8\ \mathrm{M}$$, what happens to $$[N_2O_4]$$?

Accepted Answer

$$[N_2O_4]$$ increases

Question 3

For the reaction $$2NH_3(g) \rightleftharpoons N_2$(g) + 3H_2(g)$$, which change will NOT increase the amount of ammonia in the equilibrium mixture?

Accepted Answer

Heating up the reaction

Question 4

Which of the following statements about the effect of a catalyst on a chemical equilibrium is correct?

Accepted Answer

A catalyst has no effect on the equilibrium concentrations of reactants and products

Question 5

Consider the equilibrium $$CO(g) + 2H_2(g) \rightleftharpoons CH_3OH(g). $$What is the effect of removing $$CH_3OH$$ from the system?

Accepted Answer

More $$CH_3OH$$ will form

Question 6

For the reaction $$H^+(aq) + CH_3CO_2^-(aq) \rightleftharpoons CH_3CO_2H(aq)$$, what effect will adding $$NaOH$$ have on the equilibrium?

Accepted Answer

More $$H^+$$ and $$CH_3CO_2^-$$ will form

Question 7

Which of the following changes will increase the number of moles of products for the equilibrium $$Fe_3O_4(s) + 4H_2(g) \rightleftharpoons 3Fe(s) + 4H_2O(g)$$ when the volume is increased?

Accepted Answer

The number of moles of products will increase

Question 8

At high pressure, the melting point of ice decreases. This is an example of:

Accepted Answer

Le Chatelier’s Principle

Question 9

For the reaction $$CO_2(g) + Ni(s$$) \rightleftharpoons NiO(s) + CO(g)$$, K_p$ decreases with increasing temperature. What does this indicate about the reaction?

Accepted Answer

The reaction is exothermic

Question 10

Which of the following is true at equilibrium for a chemical reaction?

Accepted Answer

The rate of the forward reaction equals the rate of the reverse reaction

Question 11

Given the reaction $$A(g) + B(g) ightleftharpoons 2C(g)$$, if $$k_{forward} = 1.4 	imes 10$$^{-12}$$\ \mathrm{M$$^{-1}$$ s$$^{-1}$$}$$ and $$k_{reverse} = 2.7 	imes 10$$^{-13}$$\ \mathrm{M$$^{-1}$$ s$$^{-1}$$}$$, what is the equilibrium constant $$K_c$$?

Accepted Answer

$$5.2$$

Question 12

Which of the following will NOT affect the value of the equilibrium constant $$K$$ for a reaction?

Accepted Answer

Adding a catalyst

Question 13

For the reaction $$2NH_3(g) \rightleftharpoons N_2$(g) + 3H_2(g)$$, what is the effect of decreasing the volume of the container?

Accepted Answer

The equilibrium shifts toward $$NH_3$$

Question 14

Which of the following best explains why increasing temperature decreases the equilibrium constant $$K$$ for an exothermic reaction?

Accepted Answer

Increasing temperature increases $$k_{reverse}$$ more than $$k_{forward}$$

Question 15

Which of the following is the correct mathematical relationship for the equilibrium constant $$K_c in $$terms of rate constants?

Accepted Answer

$$K_c = \frac{k_{forward}}{k_{reverse}}$$

Question 16

A reaction is at equilibrium. Which of the following statements is true?

Accepted Answer

The concentrations of reactants and products remain constant over time

Chemical Equilibrium: Principles, Manipulation, and Kinetic Relationships

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