Question 1

Which of the following can be the equilibrium constant for a reaction that does not yield a significant concentration of products?

Accepted Answer

A)   4 × 10-1
B)   1 × 10-2
C)   1 × 102
D)   1 × 10-15E) B) and C)
F) C) and D)

Question 2

Which of the following is the study of the rates of chemical reactions?

Accepted Answer

A)   kinetics
B)   stoichiometry
C)   thermodynamics
D)   none of theseE) A) and D)
F) B) and D)

Question 3

For the exothermic reaction 3 B)  lowering the temperature and removing NH3 C)  raising the temperature and adding NH3 and lowering the temperature and removing NH3 D)  none of these" class="answers-bank-image d-inline" rel="preload" > making which of the following changes will ensure that the reaction will not shift either to the left or to the right?

Accepted Answer

A)   raising the temperature and adding NH3
B)   lowering the temperature and removing NH3
C)   raising the temperature and adding NH3 and lowering the temperature and removing NH3
D)   none of theseE) A) and D)
F) All of the above

Question 4

For the reaction 2]2 [O2]/[H2O] B)  K = [H2O]2/[H2]2 [O2] C)  K = [H2O]2/[H2][O2] D)  K = [H2]2[O2]/[H2O]2" class="answers-bank-image d-inline" rel="preload" > , which of the following is the equilibrium constant expression?

Accepted Answer

A)   K = [H2]2 [O2]/[H2O]
B)   K = [H2O]2/[H2]2 [O2]
C)   K = [H2O]2/[H2][O2]
D)   K = [H2]2[O2]/[H2O]2E) B) and D)
F) B) and C)

Question 5

Which of the following is an example of an equilibrium situation?

Accepted Answer

A)   an unsaturated solution
B)   a saturated solution
C)   a supersaturated solution
D)   all of theseE) None of the above
F) C) and D)

Question 6

If a reaction occurs very rapidly even at a relatively low temperature, which of the following is true?

Accepted Answer

A)   The reaction is endothermic.
B)   The reaction is exothermic.
C)   The reaction has a low activation energy.
D)   The reaction must be a single-step reaction.E) A) and B)
F) A) and D)

Question 7

For the reaction 2] =0.0400 M, [N2] = 0.0200 M, and [NH3] = 1.074 × 10-7M. What is the equilibrium constant for this reaction? A)  4.69 × 10-4 B)  9.012 × 10-9 C)  6.21 × 10-10 D)  7.41 × 10-11" class="answers-bank-image d-inline" rel="preload" > equilibrium is established at 472°C when [H2] =0.0400 M, [N2] = 0.0200 M, and [NH3] = 1.074 × 10-7M. What is the equilibrium constant for this reaction?

Accepted Answer

A)   4.69 × 10-4
B)   9.012 × 10-9
C)   6.21 × 10-10
D)   7.41 × 10-11E) B) and C)
F) All of the above

Question 8

In a particular chemical reaction, two bonds are broken and no bonds are formed. Based on this information alone, which of the following is true?

Accepted Answer

A)   The reaction has a high activation energy.
B)   The reaction is endothermic.
C)   The reaction is exothermic.
D)   We cannot determine which of the statements is true.E) None of the above
F) A) and B)

Question 9

Which of the following symbols is used to denote a reversible reaction?

Accepted Answer

A)   →
B)   ←
C)   ⇌
D)   ↔E) B) and C)
F) A) and B)

Question 10

How does a decrease in temperature affect an endothermic reaction that has not reached equilibrium?

Accepted Answer

A)   The rate of reaction slows, and less product is formed.
B)   The rate of reaction slows, but more product is formed.
C)   The rate of reaction speeds up, but less product is formed.
D)   The rate of reaction speeds up, and more product is formed.E) A) and B)
F) All of the above

Question 11

Which of the following is true of activation energy?

Accepted Answer

A)   Reactions with low activation energies are rapid.
B)   The activation energy for an exothermic reaction is negative.
C)   The activation energy is the energy difference between the reactants and the products.
D)   Reactions with low activation energies have lower number of effective collisions.E) A) and C)
F) All of the above

Question 12

For the reaction 2HgO(s)  → 2Hg(l)  + O2(g) , we measure the evolution of gas to determine the rate of reaction. At the beginning of the reaction (at 0 min) , 0.070 L of O2 is present. After 15 min, the volume of O2 is 0.40 L. What is the rate of reaction?

Accepted Answer

A)   0.022 L/min
B)   0.033 L/min
C)   0.23 L/min
D)   0.33 L/minE) A) and D)
F) B) and D)

Question 13

Consider a reaction such as A2(g)  + B2(g)  → 2AB(g) . What can we say about the mechanism of the reaction?

Accepted Answer

A)   If the reaction is fast, it occurs in a single step.
B)   If the reaction is fast, it occurs in multiple steps.
C)   If the reaction is slow, it occurs in multiple steps.
D)   We must examine each case individually.E) A) and B)
F) All of the above

Question 14

Consider the following graph. 2H5OH, how would the graph change if this line represented CH3COOH? A)  The slope of the line would greater. B)  The slope of the line would be less. C)  The line would be the same. D)  This condition cannot be predicted." class="answers-bank-image d-inline" rel="preload" > The graph is based on data collected from the following reaction. 2H5OH, how would the graph change if this line represented CH3COOH? A)  The slope of the line would greater. B)  The slope of the line would be less. C)  The line would be the same. D)  This condition cannot be predicted." class="answers-bank-image d-inline" rel="preload" > If Curve B presently represents C2H5OH, how would the graph change if this line represented CH3COOH?

Accepted Answer

A)   The slope of the line would greater.
B)   The slope of the line would be less.
C)   The line would be the same.
D)   This condition cannot be predicted.E) A) and D)
F) B) and C)

Question 15

Acetic acid is the active ingredient in vinegar. In a solution of acetic acid, the following equilibrium is established. -5. What is the equilibrium constant for the following reaction?   A)  1.8 × 10-5 B)  4.2 × 10-3 C)  6.6 × 104 D)  3.1 × 109" class="answers-bank-image d-inline" rel="preload" > The equilibrium constant for this reaction is 1.5 × 10-5. What is the equilibrium constant for the following reaction? -5. What is the equilibrium constant for the following reaction?   A)  1.8 × 10-5 B)  4.2 × 10-3 C)  6.6 × 104 D)  3.1 × 109" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   1.8 × 10-5
B)   4.2 × 10-3
C)   6.6 × 104
D)   3.1 × 109E) None of the above
F) A) and C)

Question 16

The temperature effect on reaction rate is the result of which of the following?

Accepted Answer

A)   At higher temperatures, there are more collisions.
B)   At higher temperatures, a larger fraction of the collisions are effective collisions.
C)   At higher temperatures, there are more collisions and a larger fraction of the collisions are effective collisions.
D)   None of these.E) All of the above
F) B) and C)

Question 17

If a particular reactant is involved in the slowest step of a multistep reaction, then what will be the effect of increasing its concentration?

Accepted Answer

A)   The reaction rate will decrease.
B)   The reaction rate will increase.
C)   The reaction rate will be unaffected.D) B) and C)
E) A) and B)

Question 18

The rate of reaction for the decomposition of hydrogen peroxide to yield water and oxygen is represented by the following equation: Rate = k[H2O2]. Which of the following is indicated by this equation?

Accepted Answer

A)   The rate of the reaction is unaffected by the concentration of O2.
B)   The rate of the reaction will increase with the increasing concentration of H2O2.
C)   The rate of the reaction will decrease with the increasing concentration of O2.
D)   None of these are indicated by the equation.E) C) and D)
F) None of the above

Question 19

Given that the reaction 2Na2O (s)  → 4Na(s)  + 2O2(g)  is endothermic, which of the following is true of the reaction 4Na(s)  + 2O2(g)  → 2Na2O(s) ?

Accepted Answer

A)   Its activation energy is lower than that of 2Na2O(s)  → 4Na(s)  + 2O2(g) .
B)   Its activation energy is the same as that of 2Na2O(s)  → 4Na(s)  + 2O2(g) .
C)   Its activation energy is higher than that of 2Na2O(s)  → 4Na(s)  + 2O2(g) .
D)   There is no relationship between its activation energy and that of 2Na2O(s)  → 4Na(s)  + 2O2(g) .E) All of the above
F) A) and D)

Question 20

What is the effect of decreasing the temperature at which a reaction is carried out?

Accepted Answer

A)   In all cases, the rate of reaction decreases.
B)   In virtually all cases, the rate of reaction decreases.
C)   In all cases, the rate of reaction increases.
D)   In virtually all cases, the rate of reaction increases.E) None of the above
F) B) and C)

Exam 7: Reaction Rates and Chemical Equilibrium

For the reaction equilibrium is established at 472°C when [H2] =0.0400 M, [N2] = 0.0200 M, and [NH3] = 1.074 × 10-7M. What is the equilibrium constant for this reaction?

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If a particular reactant is involved in the slowest step of a multistep reaction, then what will be the effect of increasing its concentration?

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Consider a reaction such as A2(g) + B2(g) → 2AB(g) . What can we say about the mechanism of the reaction?

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If a reaction occurs very rapidly even at a relatively low temperature, which of the following is true?

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Given that the reaction 2Na2O (s) → 4Na(s) + 2O2(g) is endothermic, which of the following is true of the reaction 4Na(s) + 2O2(g) → 2Na2O(s) ?

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The rate of reaction for the decomposition of hydrogen peroxide to yield water and oxygen is represented by the following equation: Rate = k[H2O2]. Which of the following is indicated by this equation?

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The temperature effect on reaction rate is the result of which of the following?

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Acetic acid is the active ingredient in vinegar. In a solution of acetic acid, the following equilibrium is established. The equilibrium constant for this reaction is 1.5 × 10-5. What is the equilibrium constant for the following reaction?

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Which of the following is the study of the rates of chemical reactions?

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What is the effect of decreasing the temperature at which a reaction is carried out?

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For the reaction 2HgO(s) → 2Hg(l) + O2(g) , we measure the evolution of gas to determine the rate of reaction. At the beginning of the reaction (at 0 min) , 0.070 L of O2 is present. After 15 min, the volume of O2 is 0.40 L. What is the rate of reaction?

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Which of the following symbols is used to denote a reversible reaction?

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Which of the following can be the equilibrium constant for a reaction that does not yield a significant concentration of products?

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For the exothermic reaction making which of the following changes will ensure that the reaction will not shift either to the left or to the right?

Correct AnswerverifiedShow Answer

Consider the following graph. The graph is based on data collected from the following reaction. If Curve B presently represents C2H5OH, how would the graph change if this line represented CH3COOH?

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How does a decrease in temperature affect an endothermic reaction that has not reached equilibrium?

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Which of the following is an example of an equilibrium situation?

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For the reaction , which of the following is the equilibrium constant expression?

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Which of the following is true of activation energy?

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In a particular chemical reaction, two bonds are broken and no bonds are formed. Based on this information alone, which of the following is true?

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For the reaction equilibrium is established at 472°C when [H₂] =0.0400 M, [N₂] = 0.0200 M, and [NH₃] = 1.074 × 10^-7M. What is the equilibrium constant for this reaction?

Correct Answer
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Consider a reaction such as A₂(g) + B₂(g) → 2AB(g) . What can we say about the mechanism of the reaction?

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Correct Answer
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Given that the reaction 2Na₂O (s) → 4Na(s) + 2O₂(g) is endothermic, which of the following is true of the reaction 4Na(s) + 2O₂(g) → 2Na₂O(s) ?

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The rate of reaction for the decomposition of hydrogen peroxide to yield water and oxygen is represented by the following equation: Rate = k[H₂O₂]. Which of the following is indicated by this equation?

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Correct Answer
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Acetic acid is the active ingredient in vinegar. In a solution of acetic acid, the following equilibrium is established. The equilibrium constant for this reaction is 1.5 × 10^-5. What is the equilibrium constant for the following reaction?

Correct Answer
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Correct Answer
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Correct Answer
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For the reaction 2HgO(s) → 2Hg(l) + O₂(g) , we measure the evolution of gas to determine the rate of reaction. At the beginning of the reaction (at 0 min) , 0.070 L of O₂ is present. After 15 min, the volume of O₂ is 0.40 L. What is the rate of reaction?

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Consider the following graph. The graph is based on data collected from the following reaction. If Curve B presently represents C₂H₅OH, how would the graph change if this line represented CH₃COOH?

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Correct Answer
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