Question 1

What is the overall order of the following reaction, given the rate law? NO(g)+ O3(g)→ NO2(g)+ O2(g)Rate = k[NO][O3]

Accepted Answer

A) 1st order 
B) 2nd order 
C) 3rd order 
D) 1   order 
E) 0th order 
A) 1st order 
B) 2nd order 
C) 3rd order 
D) 1   order 
E) 0th order

Question 2

Which of the following is the characteristic of a zero-order reaction having only one reactant?

Accepted Answer

A) The rate of the reaction is not proportional to the concentration of the reactant. 
B) The rate of the reaction is proportional to the square of the concentration of the reactant. 
C) The rate of the reaction is proportional to the square root of the concentration of the reactant. 
D) The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. 
E) The rate of the reaction is directly proportional to the concentration of the reactant. 
A) The rate of the reaction is not proportional to the concentration of the reactant. 
B) The rate of the reaction is proportional to the square of the concentration of the reactant. 
C) The rate of the reaction is proportional to the square root of the concentration of the reactant. 
D) The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. 
E) The rate of the reaction is directly proportional to the concentration of the reactant.

Question 3

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

Accepted Answer

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

Question 4

The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 mol L-1. What is the rate constant for this reaction?

Accepted Answer

A) 1.0 × 10-2 L mol-1 s-1 
B) 4.5 × 10-2 L mol-1 s-1 
C) 9.7 × 10-2 L mol-1 s-1 
D) 2.2 × 10-2 L mol-1 s-1 
E) 3.8 × 10-2 L mol-1 s-1 
A) 1.0 × 10-2 L mol-1 s-1 
B) 4.5 × 10-2 L mol-1 s-1 
C) 9.7 × 10-2 L mol-1 s-1 
D) 2.2 × 10-2 L mol-1 s-1 
E) 3.8 × 10-2 L mol-1 s-1

Question 5

What are the units of k in the following rate law? Rate = k[X][Y]1/2

Accepted Answer

A) mol L-1 s-1 
B) L mol-1 s-1 
C) L mol-1/2 s-1 
D) L1/2 mol-1/2 s-1 
E) L mol-1 s-1/2 
A) mol L-1 s-1 
B) L mol-1 s-1 
C) L mol-1/2 s-1 
D) L1/2 mol-1/2 s-1 
E) L mol-1 s-1/2

Question 6

Match the following.

-A

Accepted Answer

A) activation energy 
B) half-life 
C) reaction order 
D) rate constant 
E) frequency factor 
A) activation energy 
B) half-life 
C) reaction order 
D) rate constant 
E) frequency factor

Question 7

Explain what the exponential factor in the Arrhenius equation represents.

Accepted Answer

The exponential factor depends on both t

Question 8

Given the following proposed mechanism, predict the rate law for the overall reaction. 2NO2 + Cl2 → 2NO2Cl (overall reaction)
Mechanism
NO2 + Cl2 → NO2Cl + Cl slow
NO2 + Cl → NO2Cl fast

Accepted Answer

A) Rate = k[NO2][Cl2] 
B) Rate = k[NO2]2[Cl2] 
C) Rate = k[NO2][Cl] 
D) Rate = k[NO2Cl][Cl] 
E) Rate = k[NO2Cl]2 
A) Rate = k[NO2][Cl2] 
B) Rate = k[NO2]2[Cl2] 
C) Rate = k[NO2][Cl] 
D) Rate = k[NO2Cl][Cl] 
E) Rate = k[NO2Cl]2

Question 9

The half-life for the decay of radium is 1620 years. What is the rate constant for this first-order process?

Accepted Answer

A) 4.28 × 10-4 yr-1 
B) 1.12 × 10-4 yr-1 
C) 2.33 × 10-4 yr-1 
D) 8.91 × 10-4 yr-1 
E) 6.17 × 10-4 yr-1 
A) 4.28 × 10-4 yr-1 
B) 1.12 × 10-4 yr-1 
C) 2.33 × 10-4 yr-1 
D) 8.91 × 10-4 yr-1 
E) 6.17 × 10-4 yr-1

Question 10

A particular first-order reaction has a rate constant of 1.35 × 102 s-1 at 25.0 °C. What is the magnitude of k at 95.0 °C if Ea = 55.5 kJ mol-1?

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 × 102 s-1 
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 × 102 s-1

Question 11

Carbon-14, which is present in all living tissue, radioactively decays via a first-order process. A one-gram sample of wood taken from a living tree gives a rate for carbon-14 decay of 13.6 counts per minute. If the half-life for carbon-14 is 5720 years, how old is a wood sample that gives a rate for carbon-14 decay of 11.9 counts per minute?

Accepted Answer

A) 5.3 × 102 yr 
B) 7.6 × 102 yr 
C) 1.1 × 103 yr 
D) 9.4 × 103 yr 
A) 5.3 × 102 yr 
B) 7.6 × 102 yr 
C) 1.1 × 103 yr 
D) 9.4 × 103 yr

Question 12

Which of the following statements is FALSE?

Accepted Answer

A) The average rate of a reaction decreases during a reaction. 
B) It is not possible to determine the rate of a reaction from its balanced equation. 
C) The rate of zero-order reactions is not dependent on concentration. 
D) The half-life of a first-order reaction is dependent on the initial concentration of reactant. 
E) None of the above statements is false. 
A) The average rate of a reaction decreases during a reaction. 
B) It is not possible to determine the rate of a reaction from its balanced equation. 
C) The rate of zero-order reactions is not dependent on concentration. 
D) The half-life of a first-order reaction is dependent on the initial concentration of reactant. 
E) None of the above statements is false.

Question 13

A reaction with an activation energy of 71.6 kJ mol-1 has a rate constant of 5.30 × 10 -6 L mol-1 s-1 at 298 K. At what temperature will the rate constant be 0.530 L mol-1 s-1?

Accepted Answer

A) 461 K 
B) 410 K 
C) 310 K 
D) 345 K 
E) 328 K 
A) 461 K 
B) 410 K 
C) 310 K 
D) 345 K 
E) 328 K

Question 14

Given the following balanced equation, determine the rate of reaction with respect to [O3]. If the rate of floss of O3 is 3.91 × 10-1 mol L-1 s-1, what is the rate of the loss of O3? 2O3(g)→ 3O2(g)

Accepted Answer

A) 2.61 mol L-1 s-1 
B) 0.937 mol L-1 s-1 
C) 0.261 mol L-1 s-1 
D) 0.587 mol L-1 s-1 
E) 0.817 mol L-1 s-1 
A) 2.61 mol L-1 s-1 
B) 0.937 mol L-1 s-1 
C) 0.261 mol L-1 s-1 
D) 0.587 mol L-1 s-1 
E) 0.817 mol L-1 s-1

Question 15

The combustion of ethylene proceeds by the reaction C2H4(g)+ 3O2(g)→ 2CO2(g)+ 2H2O(g)
When the rate of disappearance of O2 is 0.23 mol L-1 s-1, the rate of disappearance of C2H4 is ________ mol L-1 s-1.

Accepted Answer

A) 0.15 
B) 0.077 
C) 0.69 
D) 0.35 
E) 0.46 
A) 0.15 
B) 0.077 
C) 0.69 
D) 0.35 
E) 0.46

Question 16

Determine the missing initial rate for a reaction with an order of   given the following information:

Accepted Answer

A) 6.0 × 10-3 mol L-1 s-1 
B) 2.8 × 10-2 mol L-1 s-1 
C) 7.3 × 10-3 mol L-1 s-1 
D) 9.74 × 10-3 mol L-1 s-1 
E) 1.0 × 10-2 mol L-1 s-1 
A) 6.0 × 10-3 mol L-1 s-1 
B) 2.8 × 10-2 mol L-1 s-1 
C) 7.3 × 10-3 mol L-1 s-1 
D) 9.74 × 10-3 mol L-1 s-1 
E) 1.0 × 10-2 mol L-1 s-1

Question 17

The rate constant for a second-order reaction is 0.54 L mol-1 s-1. What is the half-life of this reaction if the initial concentration is 0.27 mol L-1?

Accepted Answer

A) 2.0 s 
B) 5.0 s 
C) 0.25 s 
D) 6.9 s 
E) 1.3 s 
A) 2.0 s 
B) 5.0 s 
C) 0.25 s 
D) 6.9 s 
E) 1.3 s

Question 18

How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value?

Accepted Answer

A) 6 
B) 5 
C) 7 
D) 6.5 
E) 7.5 
A) 6 
B) 5 
C) 7 
D) 6.5 
E) 7.5

Question 19

What is the overall order of the following reaction, given the rate law? X + 2 Y → 4 Z Rate = k[X][Y]

Accepted Answer

A) 3rd order 
B) 5th order 
C) 2nd order 
D) 1st order 
E) 0th order 
A) 3rd order 
B) 5th order 
C) 2nd order 
D) 1st order 
E) 0th order

Question 20

Define activation energy.

Accepted Answer

The activation energ

Exam 13: Chemical Kinetics

What is the overall order of the following reaction, given the rate law? NO(g)+ O3(g)→ NO2(g)+ O2(g)Rate = k[NO][O3]

Which of the following is the characteristic of a zero-order reaction having only one reactant?

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

The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 mol L-1. What is the rate constant for this reaction?

What are the units of k in the following rate law? Rate = k[X][Y]1/2

Match the following. -A

Explain what the exponential factor in the Arrhenius equation represents.

Given the following proposed mechanism, predict the rate law for the overall reaction. 2NO2 + Cl2 → 2NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast

The half-life for the decay of radium is 1620 years. What is the rate constant for this first-order process?

A particular first-order reaction has a rate constant of 1.35 × 102 s-1 at 25.0 °C. What is the magnitude of k at 95.0 °C if Ea = 55.5 kJ mol-1?

Which of the following statements is FALSE?

A reaction with an activation energy of 71.6 kJ mol-1 has a rate constant of 5.30 × 10 -6 L mol-1 s-1 at 298 K. At what temperature will the rate constant be 0.530 L mol-1 s-1?

Given the following balanced equation, determine the rate of reaction with respect to [O3]. If the rate of floss of O3 is 3.91 × 10-1 mol L-1 s-1, what is the rate of the loss of O3? 2O3(g)→ 3O2(g)

The combustion of ethylene proceeds by the reaction C2H4(g)+ 3O2(g)→ 2CO2(g)+ 2H2O(g) When the rate of disappearance of O2 is 0.23 mol L-1 s-1, the rate of disappearance of C2H4 is ________ mol L-1 s-1.

Determine the missing initial rate for a reaction with an order of given the following information:

The rate constant for a second-order reaction is 0.54 L mol-1 s-1. What is the half-life of this reaction if the initial concentration is 0.27 mol L-1?

How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value?

What is the overall order of the following reaction, given the rate law? X + 2 Y → 4 Z Rate = k[X][Y]

Define activation energy.

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What is the overall order of the following reaction, given the rate law? NO(g)+ O₃(g)→ NO₂(g)+ O₂(g)Rate = k[NO][O₃]

The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 mol L^-1. What is the rate constant for this reaction?

What are the units of k in the following rate law? Rate = k[X][Y]^1/2

Given the following proposed mechanism, predict the rate law for the overall reaction. 2NO₂ + Cl₂ → 2NO₂Cl (overall reaction) Mechanism NO₂ + Cl₂ → NO₂Cl + Cl slow NO₂ + Cl → NO₂Cl fast

A particular first-order reaction has a rate constant of 1.35 × 10² s^-1 at 25.0 °C. What is the magnitude of k at 95.0 °C if E_a = 55.5 kJ mol^-1?

A reaction with an activation energy of 71.6 kJ mol^-1 has a rate constant of 5.30 × 10 ^-6 L mol^-1 s^-1 at 298 K. At what temperature will the rate constant be 0.530 L mol^-1 s^-1?

Given the following balanced equation, determine the rate of reaction with respect to [O₃]. If the rate of floss of O₃ is 3.91 × 10^-1 mol L^-1 s^-1, what is the rate of the loss of O₃? 2O₃(g)→ 3O₂(g)

The combustion of ethylene proceeds by the reaction C₂H₄(g)+ 3O₂(g)→ 2CO₂(g)+ 2H₂O(g) When the rate of disappearance of O₂ is 0.23 mol L^-1 s^-1, the rate of disappearance of C₂H₄ is ________ mol L^-1 s^-1.

The rate constant for a second-order reaction is 0.54 L mol^-1s^-1. What is the half-life of this reaction if the initial concentration is 0.27 mol L^-1?