Question 1

refer to the reaction:
NO(g)  + O3(g)   →\rightarrow→ NO2(g)  + O2(g) 
for which the following rate data were obtained.
 3(g)   \rightarrow NO2(g)  + O2(g)  for which the following rate data were obtained.    -If these data were obtained by watching the rate at which NO disappears, what would be the initial instantaneous rate of disappearance of O3 in Trial 3? A)  1.6 x 10-5 M/s B)  3.2 x 10-5 M/s C)  4.8 x 10-5 M/s D)  9.6 x 10-5 M s E)  14.4 x 10-5 M/s " class="answers-bank-image d-inline" rel="preload" >
-If these data were obtained by watching the rate at which NO disappears, what would be the initial instantaneous rate of disappearance of O3 in
Trial 3?

Accepted Answer

A)   1.6 x 10-5 M/s
B)   3.2 x 10-5 M/s
C)   4.8 x 10-5 M/s
D)   9.6 x 10-5 M s
E)   14.4 x 10-5 M/s F) B) and C)
G) B) and E)

Question 2

H2 and O2 can react explosively. However, a mixture of H2 and O2 can exist indefinitely at room temperature with no reaction occurring. Explain why hydrogen and oxygen do not react under these conditions.

Accepted Answer

The activation energ...

Question 3

refer to the reaction
2 N2O5(g)   →\rightarrow→  4 NO2(g)  + O2(g) 
for which the following data were obtained.
 2O5(g)   \rightarrow  4 NO2(g)  + O2(g)  for which the following data were obtained.    -The half-life for this reaction is: A)  between 0 and 12 s B)  between 12 and 120 s C)  between 120 and 1200 s D)  between 1200 and 12,000 s E)  between 12,000 and 120,000 s " class="answers-bank-image d-inline" rel="preload" >
-The half-life for this reaction is:

Accepted Answer

A)   between 0 and 12 s
B)   between 12 and 120 s
C)   between 120 and 1200 s
D)   between 1200 and 12,000 s
E)   between 12,000 and 120,000 s F) B) and E)
G) C) and D)

Question 4

Use the following data on the initial rate of reaction to determine the overall order of the reaction.

Accepted Answer

A)   first-order overall
B)   second-order overall
C)   third-order overall
D)   fourth-order overall
E)   none of theseF) D) and E)
G) A) and B)

Question 5

Sum the following elementary steps in a mechanism to determine the stoichiometry of the overall reaction.
Cl2(g)    →\rightarrow→  2Cl(g) 
Cl(g)  + CO(g)     →\rightarrow→  COCl(g) 
COCl(g)  + Cl(g)    →\rightarrow→  COCl2(g)

Accepted Answer

A)   Cl2(g)  + 2 CO(g)  + 2 Cl(g)    →\rightarrow→  2 COCl2(g) 
B)   2 Cl2(g)  + CO(g)    →\rightarrow→  COCl2(g)  + 2 Cl(g) 
C)   2 Cl(g)  + CO(g)    →\rightarrow→  COCl2(g) 
D)   Cl2(g)  + CO(g)  + Cl(g)    →\rightarrow→  COCl2(g)  + COCl(g) 
E)   none of these F) B) and D)
G) C) and D)

Question 6

The activation energy was measured for both the forward (Ea=150 kJ/molrxn)  and reverse (Ea = 95 kJ/molrxn)  directions of a reversible reaction. What would be the activation energy for the reverse reaction in the presence of a catalyst that decreased the activation energy for the forward reaction to
125 kJ/ molrxn?

Accepted Answer

A)   25 kJ/molrxn
B)   75 kJ/ molrxn
C)   120 kJ/ molrxn
D)   30 kJ/ molrxn
E)   none of theseF) None of the above
G) A) and B)

Question 7

refer to the following reaction for the decomposition of H2O2.
2 H2O2(aq)   →\rightarrow→  2 H2O(l)  + O2(g) 
The following data were obtained
 2O2. 2 H2O2(aq)   \rightarrow  2 H2O(l)  + O2(g)  The following data were obtained    -The rate law for this reaction is: A)  zero-order in H2O2 B)  first-order in H2O2 C)  second-order in H2O2 D)  third-order in H2O2  E)  none of these " class="answers-bank-image d-inline" rel="preload" >
-The rate law for this reaction is:

Accepted Answer

A)   zero-order in H2O2
B)   first-order in H2O2
C)   second-order in H2O2
D)   third-order in H2O2 
E)   none of these F) C) and E)
G) A) and E)

Question 8

The reaction following reaction was studied at 25 2O82F1 - ? A)  trial 1 and 2 B)  trial 2 and 3 C)  trial 2 and 5 D)  trial 1 and 3 E)  none of these" class="answers-bank-image d-inline" rel="preload" > C, and the following experimental results were obtained.
2O82F1 - ? A)  trial 1 and 2 B)  trial 2 and 3 C)  trial 2 and 5 D)  trial 1 and 3 E)  none of these" class="answers-bank-image d-inline" rel="preload" > 
Which 2 trials of experimental data should be chosen to find the order of the reaction with respect to S2O82F1 - ?

Accepted Answer

A)   trial 1 and 2
B)   trial 2 and 3
C)   trial 2 and 5
D)   trial 1 and 3
E)   none of theseF) D) and E)
G) None of the above

Question 9

refer to the reaction
Cr2O72-(aq)  + 6 I-(aq)  + 14 H+(aq)  →\rightarrow→  2 Cr3+(aq)  + 3 I2(aq)  + 7 H2O(l) 
for which the following initial instantaneous rates of reaction were obtained.
 2O72-(aq)  + 6 I-(aq)  + 14 H+(aq)  \rightarrow  2 Cr3+(aq)  + 3 I2(aq)  + 7 H2O(l)  for which the following initial instantaneous rates of reaction were obtained.    -The rate law for this reaction would be: A)  zero-order in Cr2O72- B)  half-order in Cr2O72- C)  first-order in Cr2O72-  D)  second-order in Cr2O72-  E)  none of the above " class="answers-bank-image d-inline" rel="preload" >
-The rate law for this reaction would be:

Accepted Answer

A)   zero-order in Cr2O72-
B)   half-order in Cr2O72-
C)   first-order in Cr2O72- 
D)   second-order in Cr2O72- 
E)   none of the above F) None of the above
G) All of the above

Question 10

The reaction, N2O5  $\rightarrow$ NO2 + 1/2 O2, is first-order in N2O5 with a half-life of 19.25 min. How long would it take in minutes for the N2O5 concentration to decrease from 0.050 M to 0.030 M?

Accepted Answer

The answer of The reaction, N2O5  $\rightarrow$ NO2 +...

Question 11

The half-life for the first-order decomposition of nitramide, NH2NO2, into nitrous oxide, N2O, and water is 123 min at 15°C.
NH2NO2  $\rightarrow$ N2O + H2O
What is the value of the rate constant (k) for this reaction?

Accepted Answer

5.64 x 10<...

Question 12

Which equation describes the relationship between the rates at which NO is consumed and N2 is produced in the following reaction?
2 NO(g)  + 2 H2(g)    →\rightarrow→   N2(g)  + 2 H2O(g)

Accepted Answer

A)   rate N2 = rate NO
B)   rate N2 = 2(rate NO) 
C)   2(rate N2)  = rate NO
D)   (rate N2) 2 = rate NO
E)   rate N2 = (rate NO) 2 F) A) and C)
G) A) and B)

Question 13

For the reaction in the above question, how long will it take in minutes for 2.0 g of nitramide to decompose until only 0.20 g remains?

Accepted Answer

The answer of For the reaction in the above question,...

Question 14

Which of the following affect whether a collision between molecules will result in a chemical reaction?

Accepted Answer

A)   change in enthalpy for the reaction
B)   orientation of the molecules
C)   energy of the collision
D)   'b' and 'c' only
E)   all of theseF) A) and D)
G) A) and E)

Question 15

refer to the reaction
Cr2O72-(aq)  + 6 I-(aq)  + 14 H+(aq)  →\rightarrow→  2 Cr3+(aq)  + 3 I2(aq)  + 7 H2O(l) 
for which the following initial instantaneous rates of reaction were obtained.
 2O72-(aq)  + 6 I-(aq)  + 14 H+(aq)  \rightarrow  2 Cr3+(aq)  + 3 I2(aq)  + 7 H2O(l)  for which the following initial instantaneous rates of reaction were obtained.    -A graph of (Cr2O72-)  versus time would most closely resemble A)  a straight line with a negative slope. B)  a straight line with a slope of zero. C)  a straight line with a positive slope. D)  a curve in which the Cr2O72- concentration decreases rapidly at first, and then the rate at which Cr2O72- disappears slows down with time. E)  a curve in which the Cr2O72- concentration increases rapidly at first, and then the rate at which Cr2O72- appears slows down with time. " class="answers-bank-image d-inline" rel="preload" >
-A graph of (Cr2O72-)  versus time would most closely resemble

Accepted Answer

A)   a straight line with a negative slope.
B)   a straight line with a slope of zero.
C)   a straight line with a positive slope.
D)   a curve in which the Cr2O72- concentration decreases rapidly at first, and then the rate at which Cr2O72- disappears slows down with time.
E)   a curve in which the Cr2O72- concentration increases rapidly at first, and then the rate at which Cr2O72- appears slows down with time. F) All of the above
G) C) and D)

Question 16

This data applies to the next three problems.
The initial rate of disappearance of bromine (Br2)  for the reaction shown below was measured for several different concentrations of bromine, CH3COCH3, and H+ ions. (Note that H+ is a catalyst in this reaction - it participates in the reaction but is not itself consumed) 
 2)  for the reaction shown below was measured for several different concentrations of bromine, CH3COCH3, and H+ ions. (Note that H+ is a catalyst in this reaction - it participates in the reaction but is not itself consumed)     -The rate law for this reaction would be: A)  zero-order in H+ and first-order in Br2 B)  first-order in H+ and first-order in Br2 C)  first-order in H+ and zero-order in Br2 D)  second-order in H+ and zero-order in Br2 E)  none of the above." class="answers-bank-image d-inline" rel="preload" >
-The rate law for this reaction would be:

Accepted Answer

A)   zero-order in H+ and first-order in Br2
B)   first-order in H+ and first-order in Br2
C)   first-order in H+ and zero-order in Br2
D)   second-order in H+ and zero-order in Br2
E)   none of the above.F) B) and E)
G) A) and D)

Question 17

Use the following data to answer 
 These data were obtained by monitoring the rate at which the OCl- ion was consumed in the presence of a large excess of the I- ion.
OCl-(aq)  + I-(aq)   →\rightarrow→  OI-(aq)  + Cl-(aq) 
 - ion was consumed in the presence of a large excess of the I- ion. OCl-(aq)  + I-(aq)   \rightarrow  OI-(aq)  + Cl-(aq)     -What is the concentration of OCl- after 12 seconds? A)  between 1 x 10-4 and 2 x 10-4 B)  between 2 x 10-4 and 3 x 10-4 C)  between 3 x 10-4 and 4 x 10-4 D)  between 4 x 10-4 and 5 x 10-4 E)  between 5 x 10-4 and 6 x 10-4 " class="answers-bank-image d-inline" rel="preload" >
-What is the concentration of OCl- after 12 seconds?

Accepted Answer

A)   between 1 x 10-4 and 2 x 10-4
B)   between 2 x 10-4 and 3 x 10-4
C)   between 3 x 10-4 and 4 x 10-4
D)   between 4 x 10-4 and 5 x 10-4
E)   between 5 x 10-4 and 6 x 10-4 F) All of the above
G) A) and E)

Question 18

The following data table should be used to answer
Reaction: A  →\rightarrow→ B
 
-What is the half-life for this reaction, in seconds?

Accepted Answer

A)   29.1
B)   39.6
C)   47.3
D)   151
E)   none of these F) B) and E)
G) A) and E)

Question 19

This data applies to the next three problems.
The initial rate of disappearance of bromine (Br2)  for the reaction shown below was measured for several different concentrations of bromine, CH3COCH3, and H+ ions. (Note that H+ is a catalyst in this reaction - it participates in the reaction but is not itself consumed) 
 2)  for the reaction shown below was measured for several different concentrations of bromine, CH3COCH3, and H+ ions. (Note that H+ is a catalyst in this reaction - it participates in the reaction but is not itself consumed)     -The rate law for this reaction would be: A)  zero-order in CH3COCH3  B)  half-order in CH3COCH3  C)  first-order in CH3COCH3  D)  second-order in CH3COCH3  E)  none of the above." class="answers-bank-image d-inline" rel="preload" >
-The rate law for this reaction would be:

Accepted Answer

A)   zero-order in CH3COCH3 
B)   half-order in CH3COCH3 
C)   first-order in CH3COCH3 
D)   second-order in CH3COCH3 
E)   none of the above.F) B) and C)
G) All of the above

Exam 14: Kinetics

Which equation describes the relationship between the rates at which NO is consumed and N₂ is produced in the following reaction? 2 NO(g) + 2 H₂(g) $\rightarrow$ N₂(g) + 2 H₂O(g)

Correct Answer
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H₂ and O₂ can react explosively. However, a mixture of H₂ and O₂can exist indefinitely at room temperature with no reaction occurring. Explain why hydrogen and oxygen do not react under these conditions.

Correct Answer
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The activation energ...
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The half-life for the first-order decomposition of nitramide, NH₂NO₂, into nitrous oxide, N₂O, and water is 123 min at 15°C. NH₂NO₂ $\rightarrow$ N₂O + H₂O What is the value of the rate constant (k) for this reaction?

Correct Answer
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5.64 x 10<...
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Correct Answer
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Correct Answer
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For the reaction in the above question, how long will it take in minutes for 2.0 g of nitramide to decompose until only 0.20 g remains?

Correct Answer
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Sum the following elementary steps in a mechanism to determine the stoichiometry of the overall reaction. Cl₂(g) $\rightarrow$ 2Cl(g) Cl(g) + CO(g) $\rightarrow$ COCl(g) COCl(g) + Cl(g) $\rightarrow$ COCl₂(g)

Correct Answer
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Correct Answer
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Which of the following affect whether a collision between molecules will result in a chemical reaction?

Correct Answer
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Correct Answer
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Use the following data on the initial rate of reaction to determine the overall order of the reaction.

Correct Answer
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The reaction following reaction was studied at 25 C, and the following experimental results were obtained. Which 2 trials of experimental data should be chosen to find the order of the reaction with respect to S₂O₈²F1 ^- ?

Correct Answer
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The reaction, N₂O₅ $\rightarrow$ NO₂ + 1/2 O₂, is first-order in N₂O₅ with a half-life of 19.25 min. How long would it take in minutes for the N₂O₅ concentration to decrease from 0.050 M to 0.030 M?

Correct Answer
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Correct Answer
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Exam 14: Kinetics

Which equation describes the relationship between the rates at which NO is consumed and N2 is produced in the following reaction? 2 NO(g) + 2 H2(g) →\rightarrow→ N2(g) + 2 H2O(g)

Correct AnswerverifiedShow Answer

H2 and O2 can react explosively. However, a mixture of H2 and O2 can exist indefinitely at room temperature with no reaction occurring. Explain why hydrogen and oxygen do not react under these conditions.

Correct AnswerverifiedThe activation energ...View AnswerShow Answer

refer to the reaction 2 N2O5(g) →\rightarrow→ 4 NO2(g) + O2(g) for which the following data were obtained. -The half-life for this reaction is:

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refer to the following reaction for the decomposition of H2O2. 2 H2O2(aq) →\rightarrow→ 2 H2O(l) + O2(g) The following data were obtained -The rate law for this reaction is:

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refer to the reaction Cr2O72-(aq) + 6 I-(aq) + 14 H+(aq) →\rightarrow→ 2 Cr3+(aq) + 3 I2(aq) + 7 H2O(l) for which the following initial instantaneous rates of reaction were obtained. -The rate law for this reaction would be:

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refer to the reaction: NO(g) + O3(g) →\rightarrow→ NO2(g) + O2(g) for which the following rate data were obtained. -If these data were obtained by watching the rate at which NO disappears, what would be the initial instantaneous rate of disappearance of O3 in Trial 3?

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The half-life for the first-order decomposition of nitramide, NH2NO2, into nitrous oxide, N2O, and water is 123 min at 15°C. NH2NO2 →\rightarrow→ N2O + H2O What is the value of the rate constant (k) for this reaction?

Correct Answerverified5.64 x 10<...View AnswerShow Answer

Correct AnswerverifiedShow Answer

refer to the reaction Cr2O72-(aq) + 6 I-(aq) + 14 H+(aq) →\rightarrow→ 2 Cr3+(aq) + 3 I2(aq) + 7 H2O(l) for which the following initial instantaneous rates of reaction were obtained. -A graph of (Cr2O72-) versus time would most closely resemble

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

For the reaction in the above question, how long will it take in minutes for 2.0 g of nitramide to decompose until only 0.20 g remains?

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Sum the following elementary steps in a mechanism to determine the stoichiometry of the overall reaction. Cl2(g) →\rightarrow→ 2Cl(g) Cl(g) + CO(g) →\rightarrow→ COCl(g) COCl(g) + Cl(g) →\rightarrow→ COCl2(g)

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Use the following data to answer These data were obtained by monitoring the rate at which the OCl- ion was consumed in the presence of a large excess of the I- ion. OCl-(aq) + I-(aq) →\rightarrow→ OI-(aq) + Cl-(aq) -What is the concentration of OCl- after 12 seconds?

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Which of the following affect whether a collision between molecules will result in a chemical reaction?

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The following data table should be used to answer Reaction: A →\rightarrow→ B -What is the half-life for this reaction, in seconds?

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Use the following data on the initial rate of reaction to determine the overall order of the reaction.

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The reaction following reaction was studied at 25 C, and the following experimental results were obtained. Which 2 trials of experimental data should be chosen to find the order of the reaction with respect to S2O82F1 - ?

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The reaction, N2O5 →\rightarrow→ NO2 + 1/2 O2, is first-order in N2O5 with a half-life of 19.25 min. How long would it take in minutes for the N2O5 concentration to decrease from 0.050 M to 0.030 M?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Which equation describes the relationship between the rates at which NO is consumed and N₂ is produced in the following reaction? 2 NO(g) + 2 H₂(g) $\rightarrow$ N₂(g) + 2 H₂O(g)

Correct Answer
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H₂ and O₂ can react explosively. However, a mixture of H₂ and O₂can exist indefinitely at room temperature with no reaction occurring. Explain why hydrogen and oxygen do not react under these conditions.

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The activation energ...
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Correct Answer
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Correct Answer
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The half-life for the first-order decomposition of nitramide, NH₂NO₂, into nitrous oxide, N₂O, and water is 123 min at 15°C. NH₂NO₂ $\rightarrow$ N₂O + H₂O What is the value of the rate constant (k) for this reaction?

Correct Answer
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5.64 x 10<...
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Sum the following elementary steps in a mechanism to determine the stoichiometry of the overall reaction. Cl₂(g) $\rightarrow$ 2Cl(g) Cl(g) + CO(g) $\rightarrow$ COCl(g) COCl(g) + Cl(g) $\rightarrow$ COCl₂(g)

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The reaction following reaction was studied at 25 C, and the following experimental results were obtained. Which 2 trials of experimental data should be chosen to find the order of the reaction with respect to S₂O₈²F1 ^- ?

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The reaction, N₂O₅ $\rightarrow$ NO₂ + 1/2 O₂, is first-order in N₂O₅ with a half-life of 19.25 min. How long would it take in minutes for the N₂O₅ concentration to decrease from 0.050 M to 0.030 M?

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Correct Answer
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