Question 1

The half- life of a first- order reaction is 13 min. If the initial concentration of reactant is 0.085 M, it takes min for it to decrease to 0.055 M.

Accepted Answer

A)   0.048
B)   11
C)   8.4
D)   3.6
E)   8.2

Question 2

The data in the table below were obtained for the reaction:
A + B → P 
-The order of the reaction in A is .

Accepted Answer

A)   1
B)   2
C)   3
D)   4
E)   0

Question 3

The mechanism for formation of the product X is:

The intermediate reactant in the reaction is .

Accepted Answer

A)   A
B)   B
C)   C
D)   D
E)   X

Question 4

The rate limiting step in a reaction is the slowest step in the reaction sequence.

Accepted Answer

A) True 
 B)False

Question 5

A reaction was found to be third order in A. Increasing the concentration of A by a factor of 3 will cause the reaction rate to .

Accepted Answer

A)   remain constant
B)   decrease by a factor of the cube root of 3
C)   increase by a factor of 9
D)   increase by a factor of 27
E)   triple D

Question 6

The decomposition of N2O5 in solution in carbon tetrachloride proceeds via the reaction 2N2O5 (soln)  → 4NO2 (soln)  + O2 (soln) 
The reaction is first order and has a rate constant of 4.82 × 10- 3 s- 1 at 64°C. If the reaction is initiated with 0.058 mol in a 1.00- L vessel, how many moles remain after 151 s?

Accepted Answer

A)   0.055
B)   2.0 × 103 
C)   0.028
D)   0.060
E)   12 C

Question 7

In the Arrhenius equation, k = Ae- Ea/RT Is the frequency factor.

Accepted Answer

A)   R
B)   A
C)   Ea 
D)   e
E)   k B

Question 8

The reaction below is first order in [H2O2]:
2H2O2 (l)  - 2H2O (l)  + O2 (g) 
A solution originally at 0.600 M H2O2 is found to be 0.075 M after 54 min. The half- life for this reaction is min.

Accepted Answer

A)   28
B)   6.8
C)   18
D)   14
E)   54

Question 9

The following reaction is second order in [A] and the rate constant is 0.039 M- 1s- 1:
A - B
The concentration of A was 0.30 M at 23s. The initial concentration of A was _ M.

Accepted Answer

A)   2.4
B)   1.2 × 10- 2 
C)   3.7
D)   0.41
E)   0.27

Question 10

The concentration of S2O82- remaining at 1600 s is M.

Accepted Answer

A)   0.014
B)   0.043
C)   0.029
D)   0.064
E)   0.036

Question 11

The rate constant of a first- order process that has a half- life of 225 s is s- 1.

Accepted Answer

A)   3.08 × 10- 3
B)   0.693
C)   1.25
D)   12.5
E)   4.44 × 10- 3

Question 12

A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g)  -B(g) . The following data are obtained for [A] as the reaction proceeds: - 3 B)  4.4 × 10- 3 C)  9.90 × 10- 3 D)  454 E)  2.2 × 10- 3" class="answers-bank-image d-inline" rel="preload" >
-The average rate of disappearance of A between 10 s and 20 s is mol/s.

Accepted Answer

A)   1.1 × 10- 3
B)   4.4 × 10- 3
C)   9.90 × 10- 3
D)   454
E)   2.2 × 10- 3

Question 13

The data in the table below were obtained for the reaction:
A + B →  P 
-The overall order of the reaction is .

Accepted Answer

A)   1
B)   2
C)   3
D)   4
E)   0

Question 14

For the elementary reaction 3][CO]/[NO2][CO2] B)  2, k[NO2][CO2] C)  4, k[NO3][CO][NO2][CO2] D)  4, k[NO2][CO2]/[NO3][CO] E)  2, k[NO3][CO]" class="answers-bank-image d-inline" rel="preload" > the molecularity of the reaction is , and the rate law is rate = .

Accepted Answer

A)   2, k[NO3][CO]/[NO2][CO2]
B)   2, k[NO2][CO2]
C)   4, k[NO3][CO][NO2][CO2]
D)   4, k[NO2][CO2]/[NO3][CO]
E)   2, k[NO3][CO]

Question 15

The overall reaction order is the sum of the orders of each reactant in the rate law.

Accepted Answer

A) True 
 B)False

Question 16

If a rate law is second order (reactant) , doubling the reactant _ _ the reaction rate.

Accepted Answer

The answer of If a rate law is second order...

Question 17

The isomerization of methylisonitrile to acetonitrile CH3NC (g)  → CH3CN (g) 
Is first order in CH3NC. The rate constant for the reaction is 9.45 × 10- 5 s- 1 at 478 K. The half- life of the reaction when the initial [CH3NC] is 0.030 M is s.

Accepted Answer

A)   3.53E × 105
B)   1.36 × 10- 4
C)   7.33 × 103
D)   1.06 × 104
E)   5.29 × 103

Question 18

A reaction was found to be second order in carbon monoxide concentration. The rate of the reaction If the [CO] is doubled, with everything else kept the same.

Accepted Answer

A)   doubles
B)   remains unchanged
C)   is reduced by a factor of 2.
D)   increases by a factor of 4
E)   triples

Question 19

Which energy difference in the energy profile below corresponds to the activation energy for the forward reaction?

Accepted Answer

A)   x
B)   y
C)   x - y
D)   x + y
E)   y - x

Question 20

A particular first- order reaction has a rate constant of 1.35 × 102 s- 1 at 25°C. What is the magnitude of k at 95°C if Ea = 55.5 kJ/mol?

Accepted Answer

A)   4.33 × 1087
B)   1.36 × 102
C)   576
D)   2.85 × 104
E)   9.60 × 103

Exam 14: Chemical Kinetics

The half- life of a first- order reaction is 13 min. If the initial concentration of reactant is 0.085 M, it takes min for it to decrease to 0.055 M.

Correct Answer
verified

The data in the table below were obtained for the reaction: A + B → P -The order of the reaction in A is .

Correct Answer
verified

The mechanism for formation of the product X is: The intermediate reactant in the reaction is .

Correct Answer
verified

The rate limiting step in a reaction is the slowest step in the reaction sequence.

Correct Answer
verified

A reaction was found to be third order in A. Increasing the concentration of A by a factor of 3 will cause the reaction rate to .

Correct Answer
verified
D

Correct Answer
verified
C

In the Arrhenius equation, _k₌_Ae- Ea/RT Is the frequency factor.

Correct Answer
verified
B

The reaction below is first order in [H₂O₂]: 2H₂O₂(l) - 2H₂O (l) + O₂(g) A solution originally at 0.600 M H₂O₂is found to be 0.075 M after 54 min. The half- life for this reaction is min.

Correct Answer
verified

The following reaction is second order in [A] and the rate constant is 0.039 M^-¹s^-¹: A - B The concentration of A was 0.30 M at 23s. The initial concentration of A was _ M.

Correct Answer
verified

The concentration of S₂O₈²^-remaining at 1600 s is M.

Correct Answer
verified

The rate constant of a first- order process that has a half- life of 225 s is s^-¹.

Correct Answer
verified

A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) -B(g) . The following data are obtained for [A] as the reaction proceeds: -The average rate of disappearance of A between 10 s and 20 s is mol/s.

Correct Answer
verified

The data in the table below were obtained for the reaction: A + B → P -The overall order of the reaction is .

Correct Answer
verified

For the elementary reaction the molecularity of the reaction is , and the rate law is rate = .

Correct Answer
verified

The overall reaction order is the sum of the orders of each reactant in the rate law.

Correct Answer
verified

If a rate law is second order (reactant) , doubling the reactant _ _ the reaction rate.

Correct Answer
verified

The isomerization of methylisonitrile to acetonitrile CH₃NC (g) → CH₃CN (g) Is first order in CH₃NC. The rate constant for the reaction is 9.45 × 10^-⁵s^-¹at 478 K. The half- life of the reaction when the initial [CH₃NC] is 0.030 M is s.

Correct Answer
verified

A reaction was found to be second order in carbon monoxide concentration. The rate of the reaction If the [CO] is doubled, with everything else kept the same.

Correct Answer
verified

Which energy difference in the energy profile below corresponds to the activation energy for the forward reaction?

Correct Answer
verified

A particular first- order reaction has a rate constant of 1.35 × 10²s^-¹at 25°C. What is the magnitude of k at 95°C if E_a= 55.5 kJ/mol?

Correct Answer
verified

Exam 14: Chemical Kinetics

The half- life of a first- order reaction is 13 min. If the initial concentration of reactant is 0.085 M, it takes min for it to decrease to 0.055 M.

Correct AnswerverifiedShow Answer

The data in the table below were obtained for the reaction: A + B → P -The order of the reaction in A is .

Correct AnswerverifiedShow Answer

The mechanism for formation of the product X is: The intermediate reactant in the reaction is .

Correct AnswerverifiedShow Answer

The rate limiting step in a reaction is the slowest step in the reaction sequence.

Correct AnswerverifiedShow Answer

A reaction was found to be third order in A. Increasing the concentration of A by a factor of 3 will cause the reaction rate to .

Correct AnswerverifiedD

Correct AnswerverifiedC

In the Arrhenius equation, k = Ae- Ea/RT Is the frequency factor.

Correct AnswerverifiedB

The reaction below is first order in [H2O2]: 2H2O2 (l) - 2H2O (l) + O2 (g) A solution originally at 0.600 M H2O2 is found to be 0.075 M after 54 min. The half- life for this reaction is min.

Correct AnswerverifiedShow Answer

The following reaction is second order in [A] and the rate constant is 0.039 M- 1s- 1: A - B The concentration of A was 0.30 M at 23s. The initial concentration of A was _ M.

Correct AnswerverifiedShow Answer

The concentration of S2O82- remaining at 1600 s is M.

Correct AnswerverifiedShow Answer

The rate constant of a first- order process that has a half- life of 225 s is s- 1.

Correct AnswerverifiedShow Answer

A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) -B(g) . The following data are obtained for [A] as the reaction proceeds: -The average rate of disappearance of A between 10 s and 20 s is mol/s.

Correct AnswerverifiedShow Answer

The data in the table below were obtained for the reaction: A + B → P -The overall order of the reaction is .

Correct AnswerverifiedShow Answer

For the elementary reaction the molecularity of the reaction is , and the rate law is rate = .

Correct AnswerverifiedShow Answer

The overall reaction order is the sum of the orders of each reactant in the rate law.

Correct AnswerverifiedShow Answer

If a rate law is second order (reactant) , doubling the reactant _ _ the reaction rate.

Correct AnswerverifiedShow Answer

The isomerization of methylisonitrile to acetonitrile CH3NC (g) → CH3CN (g) Is first order in CH3NC. The rate constant for the reaction is 9.45 × 10- 5 s- 1 at 478 K. The half- life of the reaction when the initial [CH3NC] is 0.030 M is s.

Correct AnswerverifiedShow Answer

A reaction was found to be second order in carbon monoxide concentration. The rate of the reaction If the [CO] is doubled, with everything else kept the same.

Correct AnswerverifiedShow Answer

Which energy difference in the energy profile below corresponds to the activation energy for the forward reaction?

Correct AnswerverifiedShow Answer

A particular first- order reaction has a rate constant of 1.35 × 102 s- 1 at 25°C. What is the magnitude of k at 95°C if Ea = 55.5 kJ/mol?

Correct AnswerverifiedShow Answer

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
D

Correct Answer
verified
C

In the Arrhenius equation, _k₌_Ae- Ea/RT Is the frequency factor.

Correct Answer
verified
B

The reaction below is first order in [H₂O₂]: 2H₂O₂(l) - 2H₂O (l) + O₂(g) A solution originally at 0.600 M H₂O₂is found to be 0.075 M after 54 min. The half- life for this reaction is min.

Correct Answer
verified

The following reaction is second order in [A] and the rate constant is 0.039 M^-¹s^-¹: A - B The concentration of A was 0.30 M at 23s. The initial concentration of A was _ M.

Correct Answer
verified

The concentration of S₂O₈²^-remaining at 1600 s is M.

Correct Answer
verified

The rate constant of a first- order process that has a half- life of 225 s is s^-¹.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The isomerization of methylisonitrile to acetonitrile CH₃NC (g) → CH₃CN (g) Is first order in CH₃NC. The rate constant for the reaction is 9.45 × 10^-⁵s^-¹at 478 K. The half- life of the reaction when the initial [CH₃NC] is 0.030 M is s.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

A particular first- order reaction has a rate constant of 1.35 × 10²s^-¹at 25°C. What is the magnitude of k at 95°C if E_a= 55.5 kJ/mol?

Correct Answer
verified