Question 1

For an exothermic reaction, lowering the temperature of the reaction will ________.

Accepted Answer

A)   increase the amount of products
B)   decrease the amount of reactants
C)   decrease the amount of products
D)   both A and B

Question 2

Removing ozone as soon as it is formed will shift the equilibrium to the right.
3O₂ (g) ⇔ 2O₃ (g)

Accepted Answer

A) True 
 B)False

Question 3

Which of the following statements best describes the rate of the forward reaction as it approaches equilibrium?

Accepted Answer

A)   The rate increases as equilibrium is approached.
B)   The rate decreases as equilibrium is approached.
C)   The rate remains constant.
D)   The rate slows down, then increases, as equilibrium is approached.

Question 4

Removing product will ________. 2SO₂ (g)  + O₂ (g)   2SO₃ (g)

Accepted Answer

A)   shift the reaction to the right
B)   shift the reaction to the left
C)   have no effect
D)   cannot be determined, since the temperature is unknown

Question 5

Match each reaction and its equilibrium concentrations with its corresponding equilibrium constant value.
-N?O5 (g)  5 (g)    2 O? (g)  +   [N?O] = 0.50 M, [O?] = 1.0 M, [N?O5] = 0.10 M A) 25 B) 12.3 C) 5.0" class="answers-bank-image d-inline" rel="preload" > 2 O? (g)  + 5 (g)    2 O? (g)  +   [N?O] = 0.50 M, [O?] = 1.0 M, [N?O5] = 0.10 M A) 25 B) 12.3 C) 5.0" class="answers-bank-image d-inline" rel="preload" > [N?O] = 0.50 M, [O?] = 1.0 M, [N?O5] = 0.10 M

Accepted Answer

A)  25
B)  12.3
C)  5.0

Question 6

Calculate the equilibrium concentration of N₂ for the following reaction.  +    The equilibrium constant Keq is 0.055 and the concentrations of  and  are 1.20 M and 0.225 M, respectively.

Accepted Answer

A)   0.0915 M
B)   0.533 M
C)   0.915 M
D)   3.41 M

Question 7

Removing ammonia as soon as it is formed will ________. N₂ (g)  + 3H₂ (g)   2NH₃ (g)

Accepted Answer

A)   shift the reaction to the right
B)   shift the reaction to the left
C)   have no effect
D)   cannot be determined, since the temperature is unknown

Question 8

Decreasing the concentration of ammonia gas will ________. 2NH₃ (g)   N₂ (g)  + 3H₂ (g)

Accepted Answer

A)   shift the reaction to the right
B)   shift the reaction to the left
C)   have no effect
D)   cannot be determined, since the temperature is unknown

Question 9

Write an expression for the equilibrium constant (Keq) for the following reaction.
HCl (g) + H₂O (l)  H₃O+ (aq)+ Cl- (aq)

Accepted Answer

Keq = [ <img  loading="lazy" src="/assets/images/blured-textbook.svg" class="d-inline m-1" alt="blured image" width="139" height="30"> ]...

Question 10

The equilibrium concentrations for the reaction at 300 K are [CL₂] = 0.75 M, [PCL₃] = 0.45 M, and [PCl5] = 0.73 M. The value of Keq is ________. CL₂ (g)  + PCL₃ (g)   PCl5 (g)

Accepted Answer

A)   2.2
B)   0.15
C)   0.048
D)   4.7

Question 11

Consider the reaction: C (s)  + CO? (g)   2 CO (g)  (endothermic) . 
Match each equilibrium change with its corresponding consequence.
-decreasing the pressure

Accepted Answer

A)  Equilibrium is shifted to the right.
B)  No effect on the equilibrium.
C)  Equilibrium is shifted to the left.

Question 12

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift.
-2 SO₃ (g)  + 2 CL₂ (g)

Accepted Answer

A)  no effect
B)  right (→) 
C)  left (←)

Question 13

At equilibrium, the amount of product present is always greater than the amount of reactant present.

Accepted Answer

A) True 
 B)False

Question 14

For an endothermic reaction, lowering the temperature of the reaction will ________.

Accepted Answer

A)   increase the amount of products
B)   decrease the amount of reactants
C)   decrease the amount of products
D)   both A and B

Question 15

Adding a catalyst to any reaction will always change the value of the equilibrium constant.

Accepted Answer

A) True 
 B)False

Question 16

The double arrow in a chemical reaction indicates that the equilibrium is established since the rate of the forward reaction is equal to the rate of the reverse reaction.

Accepted Answer

A) True 
 B)False

Question 17

If the reaction vessel is expanded, this will ________. CH₄ (g)  + 2O₂ (g)   CO₂ (g)  + 2H₂O (g)

Accepted Answer

A)   shift the reaction to the right
B)   shift the reaction to the left
C)   have no effect
D)   cannot be determined, since the temperature is unknown

Question 18

The solubility of SrF₂ in water (given Ksp = 2.6 × 10-9 )  is ________.

Accepted Answer

A)   4.3 × 10-4 M
B)   1.2 × 10-4 M
C)   7.6 × 10-5 M
D)   8.7 × 10-4 M

Question 19

In an exothermic reaction, adding heat will ________.

Accepted Answer

A)   increase the amount of products
B)   decrease the amount of reactants
C)   decrease the amount of products
D)   both A and B

Question 20

If the solubility of calcium fluoride is 2.0 × 10-4 M, the solubility product value is ________.

Accepted Answer

A)   1.6 × 10-12
B)   3.2 × 10-11
C)   4.0 × 10-8
D)   8.0 × 10-12

Exam 14: Chemical Equilibrium

Consider the reaction: C (s) + CO? (g) 2 CO (g) (endothermic) . Match each equilibrium change with its corresponding consequence. -decreasing the pressure

Correct AnswerverifiedShow Answer

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -2 SO₃ (g) + 2 CL₂ (g)

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In an exothermic reaction, adding heat will ________.

Correct AnswerverifiedShow Answer

For an endothermic reaction, lowering the temperature of the reaction will ________.

Correct AnswerverifiedShow Answer

Calculate the equilibrium concentration of N₂ for the following reaction. + The equilibrium constant Keq is 0.055 and the concentrations of and are 1.20 M and 0.225 M, respectively.

Correct AnswerverifiedShow Answer

Removing ozone as soon as it is formed will shift the equilibrium to the right. 3O₂ (g) ⇔ 2O₃ (g)

Correct AnswerverifiedShow Answer

The double arrow in a chemical reaction indicates that the equilibrium is established since the rate of the forward reaction is equal to the rate of the reverse reaction.

Correct AnswerverifiedShow Answer

If the reaction vessel is expanded, this will ________. CH₄ (g) + 2O₂ (g) CO₂ (g) + 2H₂O (g)

Correct AnswerverifiedShow Answer

The equilibrium concentrations for the reaction at 300 K are [CL₂] = 0.75 M, [PCL₃] = 0.45 M, and [PCl5] = 0.73 M. The value of Keq is ________. CL₂ (g) + PCL₃ (g) PCl5 (g)

Correct AnswerverifiedShow Answer

Which of the following statements best describes the rate of the forward reaction as it approaches equilibrium?

Correct AnswerverifiedShow Answer

Decreasing the concentration of ammonia gas will ________. 2NH₃ (g) N₂ (g) + 3H₂ (g)

Correct AnswerverifiedShow Answer

Match each reaction and its equilibrium concentrations with its corresponding equilibrium constant value. -N?O5 (g) 2 O? (g) + [N?O] = 0.50 M, [O?] = 1.0 M, [N?O5] = 0.10 M

Correct AnswerverifiedShow Answer

At equilibrium, the amount of product present is always greater than the amount of reactant present.

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Removing ammonia as soon as it is formed will ________. N₂ (g) + 3H₂ (g) 2NH₃ (g)

Correct AnswerverifiedShow Answer

The solubility of SrF₂ in water (given Ksp = 2.6 × 10-9 ) is ________.

Correct AnswerverifiedShow Answer

Removing product will ________. 2SO₂ (g) + O₂ (g) 2SO₃ (g)

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If the solubility of calcium fluoride is 2.0 × 10-4 M, the solubility product value is ________.

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Write an expression for the equilibrium constant (Keq) for the following reaction. HCl (g) + H₂O (l) H₃O+ (aq)+ Cl- (aq)

Correct AnswerverifiedKeq = [ ]...View AnswerShow Answer

Adding a catalyst to any reaction will always change the value of the equilibrium constant.

Correct AnswerverifiedShow Answer

For an exothermic reaction, lowering the temperature of the reaction will ________.

Correct AnswerverifiedShow Answer

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Match each reaction and its equilibrium concentrations with its corresponding equilibrium constant value. -N?O₅ (g) 2 O? (g) + [N?O] = 0.50 M, [O?] = 1.0 M, [N?O₅] = 0.10 M

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The solubility of SrF₂ in water (given Ksp = 2.6 × 10^-9 ) is ________.

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If the solubility of calcium fluoride is 2.0 × 10^-4 M, the solubility product value is ________.

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Keq = [ ]...
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