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

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

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.

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

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.

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

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?

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

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.

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

Exam 14: Chemical Kinetics

The decomposition of N₂O₅in 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^-³s^-¹at 64°C. If the reaction is initiated with 0.058 mol in a 1.00- L vessel, how many moles remain after 151 s?

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Question 1

Correct Answer:

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

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Question 2

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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 .

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Question 3

Correct Answer:

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

(Multiple Choice)

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Question 4

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.

(Multiple Choice)

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Question 5

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.

(Multiple Choice)

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Question 6

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

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Question 7

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

(Multiple Choice)

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Question 8

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.

(Multiple Choice)

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Question 9

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

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Question 10

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.

(Multiple Choice)

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Question 11

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?

(Multiple Choice)

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Question 12

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.

(Multiple Choice)

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Question 13

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

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Question 14

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

(True/False)

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Question 15

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

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Question 16

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

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Question 17

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

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Question 18

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

(True/False)

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Question 19

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.

(Multiple Choice)

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Question 20

Showing 1 - 20 of 110

Exam 14: Chemical Kinetics

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

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 .

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

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.

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.

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

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

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.

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

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.

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?

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.

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

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

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

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

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

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

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.

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

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

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.

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.

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?

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.

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