Question 1

In the Arrhenius equation,ln k = -Ea/RT + ln A,the symbol A denotes the initial concentration of A.

Accepted Answer

A) True 
 B)False

Question 2

The combustion of ethylene proceeds by the reaction 
-1   ,the rate of appearance of   Is ________   A) 0.19 B) 0.093 C) 0.84 D) 0.42 E) 0.56" class="answers-bank-image d-inline" rel="preload" > -1   ,the rate of appearance of   Is ________   A) 0.19 B) 0.093 C) 0.84 D) 0.42 E) 0.56" class="answers-bank-image d-inline" rel="preload" > (g) + -1   ,the rate of appearance of   Is ________   A) 0.19 B) 0.093 C) 0.84 D) 0.42 E) 0.56" class="answers-bank-image d-inline" rel="preload" > (g) → -1   ,the rate of appearance of   Is ________   A) 0.19 B) 0.093 C) 0.84 D) 0.42 E) 0.56" class="answers-bank-image d-inline" rel="preload" > (g) + -1   ,the rate of appearance of   Is ________   A) 0.19 B) 0.093 C) 0.84 D) 0.42 E) 0.56" class="answers-bank-image d-inline" rel="preload" > O(g) 
When the rate of disappearance of -1   ,the rate of appearance of   Is ________   A) 0.19 B) 0.093 C) 0.84 D) 0.42 E) 0.56" class="answers-bank-image d-inline" rel="preload" > Is 0.28 mol L-1 -1   ,the rate of appearance of   Is ________   A) 0.19 B) 0.093 C) 0.84 D) 0.42 E) 0.56" class="answers-bank-image d-inline" rel="preload" > ,the rate of appearance of -1   ,the rate of appearance of   Is ________   A) 0.19 B) 0.093 C) 0.84 D) 0.42 E) 0.56" class="answers-bank-image d-inline" rel="preload" > Is ________ -1   ,the rate of appearance of   Is ________   A) 0.19 B) 0.093 C) 0.84 D) 0.42 E) 0.56" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  0.19
B)  0.093
C)  0.84
D)  0.42
E)  0.56

Question 3

For the reaction 2 HgCl2 + C2O42- → products,data are:
2 + C2O42- → products,data are:   The rate law is Rate = k[HgCl2]x[C2O42-]y. Thus: A) x = 2,y = 1 B) x = 2,y = 2 C) x = 1,y = 2 D) x = 1,y = 1 E) x = 0,y = 2" class="answers-bank-image d-inline" rel="preload" >
The rate law is Rate = k[HgCl2]x[C2O42-]y. Thus:

Accepted Answer

A)  x = 2,y = 1
B)  x = 2,y = 2
C)  x = 1,y = 2
D)  x = 1,y = 1
E)  x = 0,y = 2

Question 4

The first-order reaction,SO2Cl2 → SO2 + Cl2,has a rate constant equal to 2.20 × 10-5 s-1 at 593 K.What percentage of the initial amount of SO2Cl2 will remain after 6.00 hours?

Accepted Answer

A)  1.00%
B)  37.8%
C)  40.2%
D)  62.2%

Question 5

Given the following initial rate data,calculate the specific rate constant. 2/s2  B) 1.9 M-1 s-1  C) 3.6 M s-1  D) 1.1 × 108 M2/s2  E) 3.6 M2 s-1 " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  1.9 M2/s2 
B)  1.9 M-1 s-1 
C)  3.6 M s-1 
D)  1.1 × 108 M2/s2 
E)  3.6 M2 s-1

Question 6

Which statement is INCORRECT?

Accepted Answer

A)  Activation energy is always the same for forward and reverse reaction.
B)  If the forward reaction is endothermic,the reverse will be exothermic.
C)  In an endothermic reaction,activation energy is usually greater than the enthalpy.
D)  An activated complex has higher energy than any molecule contributing to it.
E)  The activated complex will be the highest on the energy profile.

Question 7

What is the rate law for the following mechanism?
N2O + NO → N2ONO (Slow) 
N2ONO → N2 + NO2 (Fast)

Accepted Answer

A)  Rate = k[N2O]
B)  Rate = k[NO]
C)  Rate = k[N2O][NO]
D)  Rate = k[N2][NO2]
E)  Rate = k[N2ONO]

Question 8

Why is rate = k[HgCl2] 2[C2O42-] not the rate law for the following mechanism?
2 HgCl2 + C2O42- → 2 Cl- + 2 CO2 + Hg2Cl2 (overall reaction) 
HgCl2 + C2O42- ⇌ HgCl2C2O42- (fast) 
HgCl2C2O42- + C2O42- → Hg + 2 C2O4Cl2- (slow) 
Hg + HgCl2 → Hg2Cl2 (fast) 
2 C2O4Cl2- → C2O42- + 2 Cl- + 2 CO2 (fast)

Accepted Answer

A)  The rate law is not based on the slow step of the proposed mechanism.
B)  The steps do not add to the overall reaction.
C)  The rate law does not agree with the overall reaction.
D)  The exponents of HgCl2 and C2O42- are not equal.
E)  The first step is not the slow step.

Question 9

For the reaction: C2H4Br2 + 3 KI → C2H4 + 2 KBr + KI3
Initial rate data at 60 °C are:
2H4Br2 + 3 KI → C2H4 + 2 KBr + KI3 Initial rate data at 60 °C are:   The rate law is ________. A) rate = k[KI] B) rate = k[C2H4Br2] C) rate = k[KI]2  D) rate = k[KI][C2H4Br2] E) rate = k[KI][C2H4Br2]2 " class="answers-bank-image d-inline" rel="preload" >
The rate law is ________.

Accepted Answer

A)  rate = k[KI]
B)  rate = k[C2H4Br2]
C)  rate = k[KI]2 
D)  rate = k[KI][C2H4Br2]
E)  rate = k[KI][C2H4Br2]2

Question 10

The reaction A + B → C + D is second order in A and zero order in B.The value of k is 0.012 M-1 min-1.What is the rate of this reaction when [A] = 0.125 M and [B] = 0.435 M?

Accepted Answer

A)  5 × 10-4 M min-1 
B)  3.4 × 10-3 M min-1 
C)  1.3 M min-1 
D)  1.9 × 10-4 M min-1 
E)  1.5 × 10-3 M min-1

Question 11

Which of the following statements is correct?

Accepted Answer

A)  A zero order reaction depends on the concentration of reactants.
B)  A reaction rate cannot be calculated from the collision frequency alone.
C)  The activated complex is a chemical species that can be isolated and analysed.
D)  The number of collisions has no effect on the rate constant.
E)  The orientation of a collision does not affect the rate constant.

Question 12

For the reaction: C2H4Br2 + 3 KI → C2H4 + 2 KBr + KI3,when the rate of disappearance of C2H4Br2 is 2.0 × 10-5 M/s,what is the rate of disappearance of KI?

Accepted Answer

A)  0.67 × 10-5 M/s
B)  2.0 × 10-5 M/s
C)  4.0 × 10-5 M/s
D)  6.0 × 10-5 M/s
E)  1.0 × 10-5 M/s

Question 13

For the reaction: A → Products concentration-time data are:

What is the order of this reaction with respect to [A]?

Accepted Answer

A)  zero
B)  first
C)  second
D)  third
E)  none of these

Question 14

For the reaction: 2 N2O5(g) → 4 NO2(g) + O2(g) the rate law is: 
2O5(g) → 4 NO2(g) + O2(g) the rate law is:   = k[N2O5] At 300 K,the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol.What is the half-life at 310 K? A) 2.49 × 104 s B) 9.51 × 104 s C) 9.51 × 106 s D) 6.57 × 103 s E) 1.87 × 10-1 s" class="answers-bank-image d-inline" rel="preload" >= k[N2O5]
At 300 K,the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol.What is the half-life at 310 K?

Accepted Answer

A)  2.49 × 104 s
B)  9.51 × 104 s
C)  9.51 × 106 s
D)  6.57 × 103 s
E)  1.87 × 10-1 s

Question 15

The first-order reaction,2 N2O(g) → 2 N2(g) + O2(g) ,has a rate constant equal to 0.76 s-1 at 1000 K.How long will it take for the concentration of N2O to decrease to 12% of its initial concentration?

Accepted Answer

A)  0.62 s
B)  2.8 s
C)  6.3 s
D)  8.4 s

Question 16

Calculate rate constant k for a first order reaction with a half-life of 75.0 min.

Accepted Answer

A)  52.0 min-1 
B)  1.54 × 10-4 min-1 
C)  1.33 × 10-2 min-1 
D)  9.24 × 10-3 min-1 
E)  2.67 × 10-2 min-1

Question 17

The correct units of the specific rate constant for a zero order reaction are ________.

Accepted Answer

A)  L/mol s
B)  s-1 
C)  s
D)  L2/mol2 s
E)  rate is a constant,so it has no units

Question 18

A particular first-order reaction has a rate constant of 1.35 × 3 s-1 B) 2.85 × 104 s-1 C) 576 s-1 D) 4.33 × 1087 s-1 E) 1.36 ×   s-1" class="answers-bank-image d-inline" rel="preload" > 3 s-1 B) 2.85 × 104 s-1 C) 576 s-1 D) 4.33 × 1087 s-1 E) 1.36 ×   s-1" class="answers-bank-image d-inline" rel="preload" >
At 25.0 °C.What is the magnitude of k at 3 s-1 B) 2.85 × 104 s-1 C) 576 s-1 D) 4.33 × 1087 s-1 E) 1.36 ×   s-1" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  9.56 × 103 s-1
B)  2.85 × 104 s-1
C)  576 s-1
D)  4.33 × 1087 s-1
E)  1.36 × 3 s-1 
B)  2.85 × 104 s-1 
C)  576 s-1 
D)  4.33 × 1087 s-1 
E)  1.36 ×   s-1" class="answers-bank-image d-inline" rel="preload" > s-1

Question 19

The rate data from a chemical reaction shows that doubling the concentration of A with the concentration of B remaining constant causes the rate to increase by a factor of four.What is the reaction order for [A]?

Accepted Answer

A)  0
B)  0.5
C)  1
D)  2
E)  3

Question 20

If the half-life of a reaction depends on the concentration of the reactant,then the reaction cannot be ________ order.

Accepted Answer

A)  second
B)  zero
C)  first
D)  third

Exam 20: Chemical Kinetics

For the reaction: A → Products concentration-time data are: What is the order of this reaction with respect to [A]?

Correct Answer
verified

For the reaction: C₂H₄Br₂ + 3 KI → C₂H₄+ 2 KBr + KI₃,when the rate of disappearance of C₂H₄Br₂ is 2.0 × 10^-5 M/s,what is the rate of disappearance of KI?

Correct Answer
verified

The reaction A + B → C + D is second order in A and zero order in B.The value of k is 0.012 M^-1 min^-1.What is the rate of this reaction when [A] = 0.125 M and [B] = 0.435 M?

Correct Answer
verified

The correct units of the specific rate constant for a zero order reaction are ________.

Correct Answer
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The first-order reaction,2 N₂O(g) → 2 N₂(g) + O₂(g) ,has a rate constant equal to 0.76 s^-1 at 1000 K.How long will it take for the concentration of N₂O to decrease to 12% of its initial concentration?

Correct Answer
verified

Correct Answer
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A particular first-order reaction has a rate constant of 1.35 × At 25.0 °C.What is the magnitude of k at

Correct Answer
verified

In the Arrhenius equation,ln k = ^-^E_a/RT + ln A,the symbol A denotes the initial concentration of A.

Correct Answer
verified

Which statement is INCORRECT?

Correct Answer
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The first-order reaction,SO₂Cl₂ → SO₂ + Cl₂,has a rate constant equal to 2.20 × 10^-5 s^-1 at 593 K.What percentage of the initial amount of SO₂Cl₂ will remain after 6.00 hours?

Correct Answer
verified

The rate data from a chemical reaction shows that doubling the concentration of A with the concentration of B remaining constant causes the rate to increase by a factor of four.What is the reaction order for [A]?

Correct Answer
verified

The combustion of ethylene proceeds by the reaction (g) + (g) → (g) + O(g) When the rate of disappearance of Is 0.28 mol L^-1 ,the rate of appearance of Is ________

Correct Answer
verified

Given the following initial rate data,calculate the specific rate constant.

Correct Answer
verified

Calculate rate constant k for a first order reaction with a half-life of 75.0 min.

Correct Answer
verified

For the reaction: C₂H₄Br₂ + 3 KI → C₂H₄ + 2 KBr + KI₃ Initial rate data at 60 °C are: The rate law is ________.

Correct Answer
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What is the rate law for the following mechanism? N₂O + NO → N₂ONO (Slow) N₂ONO → N₂ + NO₂ (Fast)

Correct Answer
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If the half-life of a reaction depends on the concentration of the reactant,then the reaction cannot be ________ order.

Correct Answer
verified

For the reaction 2 HgCl₂ + C₂O₄^2- → products,data are: The rate law is Rate = k[HgCl₂]^x[C₂O₄^2-]^y. Thus:

Correct Answer
verified

For the reaction: 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) the rate law is: = k[N₂O₅] At 300 K,the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol.What is the half-life at 310 K?

Correct Answer
verified

Which of the following statements is correct?

Correct Answer
verified

Exam 20: Chemical Kinetics

For the reaction: A → Products concentration-time data are: What is the order of this reaction with respect to [A]?

Correct AnswerverifiedShow Answer

For the reaction: C2H4Br2 + 3 KI → C2H4 + 2 KBr + KI3,when the rate of disappearance of C2H4Br2 is 2.0 × 10-5 M/s,what is the rate of disappearance of KI?

Correct AnswerverifiedShow Answer

The reaction A + B → C + D is second order in A and zero order in B.The value of k is 0.012 M-1 min-1.What is the rate of this reaction when [A] = 0.125 M and [B] = 0.435 M?

Correct AnswerverifiedShow Answer

The correct units of the specific rate constant for a zero order reaction are ________.

Correct AnswerverifiedShow Answer

The first-order reaction,2 N2O(g) → 2 N2(g) + O2(g) ,has a rate constant equal to 0.76 s-1 at 1000 K.How long will it take for the concentration of N2O to decrease to 12% of its initial concentration?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A particular first-order reaction has a rate constant of 1.35 × At 25.0 °C.What is the magnitude of k at

Correct AnswerverifiedShow Answer

In the Arrhenius equation,ln k = -Ea/RT + ln A,the symbol A denotes the initial concentration of A.

Correct AnswerverifiedShow Answer

Which statement is INCORRECT?

Correct AnswerverifiedShow Answer

The first-order reaction,SO2Cl2 → SO2 + Cl2,has a rate constant equal to 2.20 × 10-5 s-1 at 593 K.What percentage of the initial amount of SO2Cl2 will remain after 6.00 hours?

Correct AnswerverifiedShow Answer

The rate data from a chemical reaction shows that doubling the concentration of A with the concentration of B remaining constant causes the rate to increase by a factor of four.What is the reaction order for [A]?

Correct AnswerverifiedShow Answer

The combustion of ethylene proceeds by the reaction (g) + (g) → (g) + O(g) When the rate of disappearance of Is 0.28 mol L-1 ,the rate of appearance of Is ________

Correct AnswerverifiedShow Answer

Given the following initial rate data,calculate the specific rate constant.

Correct AnswerverifiedShow Answer

Calculate rate constant k for a first order reaction with a half-life of 75.0 min.

Correct AnswerverifiedShow Answer

For the reaction: C2H4Br2 + 3 KI → C2H4 + 2 KBr + KI3 Initial rate data at 60 °C are: The rate law is ________.

Correct AnswerverifiedShow Answer

What is the rate law for the following mechanism? N2O + NO → N2ONO (Slow) N2ONO → N2 + NO2 (Fast)

Correct AnswerverifiedShow Answer

If the half-life of a reaction depends on the concentration of the reactant,then the reaction cannot be ________ order.

Correct AnswerverifiedShow Answer

For the reaction 2 HgCl2 + C2O42- → products,data are: The rate law is Rate = k[HgCl2]x[C2O42-]y. Thus:

Correct AnswerverifiedShow Answer

For the reaction: 2 N2O5(g) → 4 NO2(g) + O2(g) the rate law is: = k[N2O5] At 300 K,the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol.What is the half-life at 310 K?

Correct AnswerverifiedShow Answer

Which of the following statements is correct?

Correct AnswerverifiedShow Answer

Correct Answer
verified

For the reaction: C₂H₄Br₂ + 3 KI → C₂H₄+ 2 KBr + KI₃,when the rate of disappearance of C₂H₄Br₂ is 2.0 × 10^-5 M/s,what is the rate of disappearance of KI?

Correct Answer
verified

The reaction A + B → C + D is second order in A and zero order in B.The value of k is 0.012 M^-1 min^-1.What is the rate of this reaction when [A] = 0.125 M and [B] = 0.435 M?

Correct Answer
verified

Correct Answer
verified

The first-order reaction,2 N₂O(g) → 2 N₂(g) + O₂(g) ,has a rate constant equal to 0.76 s^-1 at 1000 K.How long will it take for the concentration of N₂O to decrease to 12% of its initial concentration?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

In the Arrhenius equation,ln k = ^-^E_a/RT + ln A,the symbol A denotes the initial concentration of A.

Correct Answer
verified

Correct Answer
verified

The first-order reaction,SO₂Cl₂ → SO₂ + Cl₂,has a rate constant equal to 2.20 × 10^-5 s^-1 at 593 K.What percentage of the initial amount of SO₂Cl₂ will remain after 6.00 hours?

Correct Answer
verified

Correct Answer
verified

The combustion of ethylene proceeds by the reaction (g) + (g) → (g) + O(g) When the rate of disappearance of Is 0.28 mol L^-1 ,the rate of appearance of Is ________

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

For the reaction: C₂H₄Br₂ + 3 KI → C₂H₄ + 2 KBr + KI₃ Initial rate data at 60 °C are: The rate law is ________.

Correct Answer
verified

What is the rate law for the following mechanism? N₂O + NO → N₂ONO (Slow) N₂ONO → N₂ + NO₂ (Fast)

Correct Answer
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Correct Answer
verified

For the reaction 2 HgCl₂ + C₂O₄^2- → products,data are: The rate law is Rate = k[HgCl₂]^x[C₂O₄^2-]^y. Thus:

Correct Answer
verified

For the reaction: 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) the rate law is: = k[N₂O₅] At 300 K,the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol.What is the half-life at 310 K?

Correct Answer
verified

Correct Answer
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