Question 1

If the activation energy for a given compound is found to be 42.0 kJ mol-1 with a frequency factor of 8.0 × 1010 s-1, what is the rate constant for this reaction at 298 K?

Accepted Answer

A) 2.9 × 10-4 s-1 
B) 7.4 × 10-4 s-1 
C) 1.4 × 109 s-1 
D) 4.6 × 10 5 s-1 
E) 3.5 × 103 s-1

Question 2

The second-order reaction 2Mn(CO)5 → Mn2(CO)10 has a rate constant equal to 3.0 × 109 L mol-1 s-1 at 25 °C. If the initial concentration of Mn(CO)5 is 2.0 × 10-5 mol L-1, how long will it take for 90.% of the reactant to disappear?

Accepted Answer

A) 6.7 × 10-16 s 
B) 7.4 × 10-15 s 
C) 1.5 × 10-4 s 
D) 6.0 × 103 s

Question 3

Identify a heterogeneous catalyst.

Accepted Answer

A) CFCs with ozone 
B) Pd in H2 gas 
C) KI dissolved in H2O2 
D) H2SO4 with concentrated HCl 
E) H3PO4 with an alcohol

Question 4

For the first-order reaction, 2N2O(g)→ 2N2(g)+ O2(g), what is the concentration of N2O after 3 half-lives if 0.25 mol of N2O is initially placed into a 1.00 L reaction vessel?

Accepted Answer

A) 1.6 × 10-2 mol L-1 
B) 3.1 × 10-2 mol L-1 
C) 6.2 × 10-2 mol L-1 
D) 1.2 × 10-1 mol L-1

Question 5

Which of the following represents the integrated rate law for a zeroth-order reaction?

Accepted Answer

A)   = -kt 
B)   -  = kt 
C) [A]t - [A]0 = -kt 
D) k = Ae(-Ea/RT) 
E)   =   + lnA

Question 6

The first-order decomposition of N2O at 1000 K has a rate constant of 0.76 s-1. If the initial concentration of N2O is 10.9 mol L-1, what is the concentration of N2O after 9.6 s?

Accepted Answer

A) 7.4 × 10-3 mol L-1 
B) 1.0 × 10-3 mol L-1 
C) 1.4 × 10-3 mol L-1 
D) 3.6 × 10-3 mol L-1 
E) 8.7 × 10-3 mol L-1

Question 7

SO2Cl2 decomposes in the gas phase by the reaction SO2Cl2(g)→ SO2(g)+ Cl2(g)
The reaction is first order in SO2Cl2 and the rate constant is 3.0 × 10-6 s-1at 600 K. A vessel is charged with 2.4 atm of SO2Cl2 at 600 K. The partial pressure of SO2Cl2 at 3.0 × 105 is ________ atm.

Accepted Answer

A) 0.76 
B) 2.2 
C) 0.98 
D) 0.29 
E) 1.4 × 105

Question 8

Determine the rate law and the value of k for the following reaction using the data provided: 2N2O5(g)→ 4NO2(g)+ O2(g)[N2O5]i (M)Initial Rate (M-1 s-1)
0.093 4.84 × 10-4
0.186 9.67 × 10-4
0.279 1.45 × 10-3

Accepted Answer

A) Rate = 5.6 × 10-2 M-1 s-1[N2O5]2 
B) Rate = 6.0 × 10-1 M-2 s-1[N2O5]3 
C) Rate = 1.6 × 10-3 M1/2 s-1[N2O5]1/2 
D) Rate = 1.7 × 10-2 M-1/2 s-1[N2O5]3/2 
E) Rate = 5.2 × 10⁻3 s-1[N2O5]

Question 9

A reaction is found to have an activation energy of 108 kJ mol-1. If the rate constant for this reaction is 4.60 × 10-6 s-1 at 275 K, what is the rate constant at 366 K?

Accepted Answer

A) 12 s-1 
B) 1.7 s-1 
C) 0.58 s-1 
D) 5.4 × 10-5 s-1 
E) 1.9 × 10-4 s-1

Question 10

Identify the rate-determining step.

Accepted Answer

A) the slowest step 
B) the faster step 
C) the fast step 
D) always the last step 
E) always the second step

Question 11

Given the following balanced equation, determine the rate of reaction with respect to [O3]. 2O3(g)→ 3O2(g)

Accepted Answer

A) Rate = -   
B) Rate = -   
C) Rate = +   
D) Rate = +   
E) It is not possible to determine the answer without more information.

Question 12

The first-order decay of radon has a half-life of 3.823 days. How many grams of radon decomposes after 5.55 days if the sample initially weighs 100.0 grams?

Accepted Answer

A) 83.4 g 
B) 16.6 g 
C) 50.0 g 
D) 36.6 g 
E) 63.4 g

Question 13

Calculate the activation energy, Ea, for a reaction with a frequency factor, A, of 6.10 × 1014 s-1 and a rate constant of 13.0 s-1 at 320 K.

Accepted Answer

A) 62.8 kJ mol-1 
B) 83.8 kJ mol-1 
C) 41.3 kJ mol-1 
D) 97.9 kJ mol-1 
E) 106 kJ mol-1

Question 14

A reaction with an activation energy of 34.0 kJ mol-1 has a rate constant of 26.8 s-1 at 354 K. What is the rate constant at 314 K?

Accepted Answer

A) 6.15 s-1 
B) 2.08 s-1 
C) 7.68 s-1 
D) 9.80 s-1 
E) 4.00 s-1

Question 15

Given the following balanced equation, determine the rate of reaction with respect to [SO3]. If the rate of O2 loss is 3.56 × 10-3 mol L-1 s-1, what is the rate of formation of SO3? 2SO2(g)+ O2(g)→ 2SO3(g)

Accepted Answer

A) 3.56 × 10-3 mol L-1 s-1 
B) 1.19 × 10-3 mol L-1 s-1 
C) 1.78 × 10-3 mol L-1 s-1 
D) 1.42 × 10-2 mol L-1 s-1 
E) 7.12 × 10-3 mol L-1 s-1

Question 16

What is a catalyst and what function does it serve?

Accepted Answer

The answer of What is a catalyst and what function...

Question 17

How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?

Accepted Answer

A) 3 
B) 1 
C) 1.75 
D) 2.75 
E) 2

Question 18

The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3 s-1. If the initial concentration of N2O5 is 2.88 mol L-1, what is the concentration of N2O5 after 12.5 minutes?

Accepted Answer

A) 0.124 mol L-1 
B) 0.805 mol L-1 
C) 2.82 mol L-1 
D) 0.355 mol L-1 
E) 0.174 mol L-1

Question 19

Determine the rate law and the value of k for the following reaction using the data provided: 2NO(g)+ O2(g)→ 2NO2(g)[NO]i (M)[O2]i (M)Initial Rate (M-1 s-1)
0.030 0.0055 8.55 × 10-3
0.030 0.0110 1.71 × 10-2
0.060 0.0055 3.42 × 10-2

Accepted Answer

A) Rate = 57 M-1 s-1[NO][O2] 
B) Rate = 3.8 M-1/2 s-1[NO][O2]1/2 
C) Rate = 3.1 × 105 M-3 s-1[NO]2[O2]2 
D) Rate = 1.7 × 103 M-2 s-1[NO]2[O2] 
E) Rate = 9.4 × 103 M-2 s-1[NO][O2]2

Question 20

Given the following balanced equation, determine the rate of reaction with respect to [O2]. 2O3(g)→ 3O2(g)

Accepted Answer

A) Rate = -  
B) Rate = -   
C) Rate = +   
D) Rate = +  
E) It is not possible to determine the answer without more information.

Exam 13: Chemical Kinetics

If the activation energy for a given compound is found to be 42.0 kJ mol^-1 with a frequency factor of 8.0 × 10¹⁰ s^-1, what is the rate constant for this reaction at 298 K?

The second-order reaction 2Mn(CO) ₅ → Mn₂(CO) ₁₀ has a rate constant equal to 3.0 × 10⁹ L mol^-1 s^-1 at 25 °C. If the initial concentration of Mn(CO) ₅ is 2.0 × 10^-5 mol L^-1, how long will it take for 90.% of the reactant to disappear?

Identify a heterogeneous catalyst.

For the first-order reaction, 2N₂O(g) → 2N₂(g) + O₂(g) , what is the concentration of N₂O after 3 half-lives if 0.25 mol of N₂O is initially placed into a 1.00 L reaction vessel?

Which of the following represents the integrated rate law for a zeroth-order reaction?

The first-order decomposition of N₂O at 1000 K has a rate constant of 0.76 s^-1. If the initial concentration of N₂O is 10.9 mol L^-1, what is the concentration of N₂O after 9.6 s?

Determine the rate law and the value of k for the following reaction using the data provided: 2N₂O₅(g) → 4NO₂(g) + O₂(g) [N₂O₅]_i (M) Initial Rate (M^-1s^-1) 0.093 4.84 × 10^-4 0.186 9.67 × 10^-4 0.279 1.45 × 10^-3

A reaction is found to have an activation energy of 108 kJ mol^-1. If the rate constant for this reaction is 4.60 × 10^-6 s^-1 at 275 K, what is the rate constant at 366 K?

Identify the rate-determining step.

Given the following balanced equation, determine the rate of reaction with respect to [O₃]. 2O₃(g) → 3O₂(g)

The first-order decay of radon has a half-life of 3.823 days. How many grams of radon decomposes after 5.55 days if the sample initially weighs 100.0 grams?

Calculate the activation energy, E_a, for a reaction with a frequency factor, A, of 6.10 × 10¹⁴ s^-1 and a rate constant of 13.0 s^-1 at 320 K.

A reaction with an activation energy of 34.0 kJ mol^-1 has a rate constant of 26.8 s^-1 at 354 K. What is the rate constant at 314 K?

Given the following balanced equation, determine the rate of reaction with respect to [SO₃]. If the rate of O₂ loss is 3.56 × 10^-3 mol L^-1 s^-1, what is the rate of formation of SO₃? 2SO₂(g) + O₂(g) → 2SO₃(g)

What is a catalyst and what function does it serve?

How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?

The first-order decomposition of N₂O₅ at 328 K has a rate constant of 1.70 × 10^-3 s^-1. If the initial concentration of N₂O₅ is 2.88 mol L^-1, what is the concentration of N₂O₅ after 12.5 minutes?

Determine the rate law and the value of k for the following reaction using the data provided: 2NO(g) + O₂(g) → 2NO₂(g) [NO]_i(M) [O₂]_i (M) Initial Rate (M^-1s^-1) 0.030 0.0055 8.55 × 10^-3 0.030 0.0110 1.71 × 10^-2 0.060 0.0055 3.42 × 10^-2

Given the following balanced equation, determine the rate of reaction with respect to [O₂]. 2O₃(g) → 3O₂(g)

Exam 13: Chemical Kinetics

If the activation energy for a given compound is found to be 42.0 kJ mol-1 with a frequency factor of 8.0 × 1010 s-1, what is the rate constant for this reaction at 298 K?

The second-order reaction 2Mn(CO) 5 → Mn2(CO) 10 has a rate constant equal to 3.0 × 109 L mol-1 s-1 at 25 °C. If the initial concentration of Mn(CO) 5 is 2.0 × 10-5 mol L-1, how long will it take for 90.% of the reactant to disappear?

Identify a heterogeneous catalyst.

For the first-order reaction, 2N2O(g) → 2N2(g) + O2(g) , what is the concentration of N2O after 3 half-lives if 0.25 mol of N2O is initially placed into a 1.00 L reaction vessel?

Which of the following represents the integrated rate law for a zeroth-order reaction?

The first-order decomposition of N2O at 1000 K has a rate constant of 0.76 s-1. If the initial concentration of N2O is 10.9 mol L-1, what is the concentration of N2O after 9.6 s?

SO2Cl2 decomposes in the gas phase by the reaction SO2Cl2(g) → SO2(g) + Cl2(g) The reaction is first order in SO2Cl2 and the rate constant is 3.0 × 10-6 s-1at 600 K. A vessel is charged with 2.4 atm of SO2Cl2 at 600 K. The partial pressure of SO2Cl2 at 3.0 × 105 is ________ atm.

Determine the rate law and the value of k for the following reaction using the data provided: 2N2O5(g) → 4NO2(g) + O2(g) [N2O5]i (M) Initial Rate (M-1 s-1) 0.093 4.84 × 10-4 0.186 9.67 × 10-4 0.279 1.45 × 10-3

A reaction is found to have an activation energy of 108 kJ mol-1. If the rate constant for this reaction is 4.60 × 10-6 s-1 at 275 K, what is the rate constant at 366 K?

Identify the rate-determining step.

Given the following balanced equation, determine the rate of reaction with respect to [O3]. 2O3(g) → 3O2(g)

The first-order decay of radon has a half-life of 3.823 days. How many grams of radon decomposes after 5.55 days if the sample initially weighs 100.0 grams?

Calculate the activation energy, Ea, for a reaction with a frequency factor, A, of 6.10 × 1014 s-1 and a rate constant of 13.0 s-1 at 320 K.

A reaction with an activation energy of 34.0 kJ mol-1 has a rate constant of 26.8 s-1 at 354 K. What is the rate constant at 314 K?

Given the following balanced equation, determine the rate of reaction with respect to [SO3]. If the rate of O2 loss is 3.56 × 10-3 mol L-1 s-1, what is the rate of formation of SO3? 2SO2(g) + O2(g) → 2SO3(g)

What is a catalyst and what function does it serve?

How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?

The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3 s-1. If the initial concentration of N2O5 is 2.88 mol L-1, what is the concentration of N2O5 after 12.5 minutes?

Determine the rate law and the value of k for the following reaction using the data provided: 2NO(g) + O2(g) → 2NO2(g) [NO]i (M) [O2]i (M) Initial Rate (M-1 s-1) 0.030 0.0055 8.55 × 10-3 0.030 0.0110 1.71 × 10-2 0.060 0.0055 3.42 × 10-2

Given the following balanced equation, determine the rate of reaction with respect to [O2]. 2O3(g) → 3O2(g)

If the activation energy for a given compound is found to be 42.0 kJ mol^-1 with a frequency factor of 8.0 × 10¹⁰ s^-1, what is the rate constant for this reaction at 298 K?

The second-order reaction 2Mn(CO) ₅ → Mn₂(CO) ₁₀ has a rate constant equal to 3.0 × 10⁹ L mol^-1 s^-1 at 25 °C. If the initial concentration of Mn(CO) ₅ is 2.0 × 10^-5 mol L^-1, how long will it take for 90.% of the reactant to disappear?

For the first-order reaction, 2N₂O(g) → 2N₂(g) + O₂(g) , what is the concentration of N₂O after 3 half-lives if 0.25 mol of N₂O is initially placed into a 1.00 L reaction vessel?

The first-order decomposition of N₂O at 1000 K has a rate constant of 0.76 s^-1. If the initial concentration of N₂O is 10.9 mol L^-1, what is the concentration of N₂O after 9.6 s?

Determine the rate law and the value of k for the following reaction using the data provided: 2N₂O₅(g) → 4NO₂(g) + O₂(g) [N₂O₅]_i (M) Initial Rate (M^-1s^-1) 0.093 4.84 × 10^-4 0.186 9.67 × 10^-4 0.279 1.45 × 10^-3

A reaction is found to have an activation energy of 108 kJ mol^-1. If the rate constant for this reaction is 4.60 × 10^-6 s^-1 at 275 K, what is the rate constant at 366 K?

Given the following balanced equation, determine the rate of reaction with respect to [O₃]. 2O₃(g) → 3O₂(g)

Calculate the activation energy, E_a, for a reaction with a frequency factor, A, of 6.10 × 10¹⁴ s^-1 and a rate constant of 13.0 s^-1 at 320 K.

A reaction with an activation energy of 34.0 kJ mol^-1 has a rate constant of 26.8 s^-1 at 354 K. What is the rate constant at 314 K?

Given the following balanced equation, determine the rate of reaction with respect to [SO₃]. If the rate of O₂ loss is 3.56 × 10^-3 mol L^-1 s^-1, what is the rate of formation of SO₃? 2SO₂(g) + O₂(g) → 2SO₃(g)

The first-order decomposition of N₂O₅ at 328 K has a rate constant of 1.70 × 10^-3 s^-1. If the initial concentration of N₂O₅ is 2.88 mol L^-1, what is the concentration of N₂O₅ after 12.5 minutes?

Determine the rate law and the value of k for the following reaction using the data provided: 2NO(g) + O₂(g) → 2NO₂(g) [NO]_i(M) [O₂]_i (M) Initial Rate (M^-1s^-1) 0.030 0.0055 8.55 × 10^-3 0.030 0.0110 1.71 × 10^-2 0.060 0.0055 3.42 × 10^-2

Given the following balanced equation, determine the rate of reaction with respect to [O₂]. 2O₃(g) → 3O₂(g)