Question 1

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

Accepted Answer

A)  M/s 
B)  M-1s-1 
C)  M1/2s-1 
D)  M-1/2s-1 
E)  M-1s-1/2

Question 2

What is the overall order of the following reaction,given the rate law?
2 X + 3 Y → 2 Z Rate = k[X]1[Y]2

Accepted Answer

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

Question 3

For a certain reaction,a plot of ln [A] vs.time gives a straight line with a slope of -1.46 s-1 and a y-intercept of 4.30.What is the order of the reaction?

Accepted Answer

A)  zeroth-order 
B)  first-order 
C)  second-order 
D)  third-order 
E)  not enough information is given to solve the problem

Question 4

Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g)+ O2(g)→ 2 NO2(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

Accepted Answer

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

Question 5

The rate constant for a second-order reaction is 0.54 M-1s-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

Accepted Answer

A)  0.089 s 
B)  1.8 s 
C)  0.31 s 
D)  5.6 s 
E)  1.3 s

Question 6

The rate constant for a first-order reaction is 0.54 s-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

Accepted Answer

A)  0.089 s 
B)  1.8 s 
C)  0.31 s 
D)  5.6 s 
E)  1.3 s

Question 7

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 M,what is the concentration of N2O5 after 12.5 minutes?

Accepted Answer

A)  0.124 M 
B)  0.805 M 
C)  2.82 M 
D)  0.355 M 
E)  0.174 M

Question 8

A reaction occurs via the following sequence of elementary steps.What is the rate law based on this reaction mechanism?
1st step: A ⇌ B very fast
2nd step: B + C → D slow
3rd step: D → 2E fast

Accepted Answer

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

Question 9

What is a catalyst and what function does it serve?

Accepted Answer

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

Question 10

Give the characteristic of a second 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.

Question 11

Write a balanced reaction for which the following rate relationships are TRUE. Rate =   =  = -

Accepted Answer

A)   N2 + O2 →     N2O 
B)  2 N2O → 2 N2 + O2 
C)  N2O → N2 + 2 O2 
D)   N2O →  N2 + O2 
E)  2 N2 + O2 → 2 N2O

Question 12

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

Accepted Answer

A)  Ms-1 
B)  Ms 
C)  M-1s-1 
D)  M-2s-1 
E)  M2s-1

Question 13

The first-order decomposition of ammonium nitrate has a rate constant of 0.110 min-1.If the initial concentration is 0.551 M,what is the concentration after 38.5 min?

Accepted Answer

A)  0.0372 M 
B)  7.98 × 10-3 M 
C)  0.513 M 
D)  0.221 M 
E)  0.143 M

Question 14

In the hydrogenation of double bonds,a catalyst is needed.In the first step,the reactants must come into contact with a metal surface.This step is known as

Accepted Answer

A)  adsorption. 
B)  diffusion. 
C)  reaction. 
D)  desorption. 
E)  none of the above.

Question 15

Define activation energy.

Accepted Answer

The answer of Define activation energy....

Question 16

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

Accepted Answer

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

Question 17

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

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 ×  s-1

Question 18

The elementary reaction  (g)→ 2NO(g)+  (g) is second order in  and the rate constant at 501 K is 7.93 × 10-3   .The reaction half-life at this temperature when  = 0.45 M is ________ s.

Accepted Answer

A)  3.6 × 10-3 
B)  0.011 
C)  126 
D)  87 
E)  280

Question 19

Give 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.

Question 20

The combustion of ethylene proceeds by the reaction C2H4(g)+ 3O2(g)→2CO2(g)+ 2H2O(g)
When the rate of disappearance of O2 is 0.28 M s-1,the rate of appearance of CO2 is ________ M s-1.

Accepted Answer

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

Exam 15: Chemical Kinetics

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

What is the overall order of the following reaction,given the rate law? 2 X + 3 Y → 2 Z Rate = k[X]¹[Y]²

For a certain reaction,a plot of ln [A] vs.time gives a straight line with a slope of -1.46 s^-1 and a y-intercept of 4.30.What is the order of the reaction?

Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g) + O₂(g) → 2 NO₂(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

The rate constant for a second-order reaction is 0.54 M^-1s^-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

The rate constant for a first-order reaction is 0.54 s^-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

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 M,what is the concentration of N₂O₅ after 12.5 minutes?

A reaction occurs via the following sequence of elementary steps.What is the rate law based on this reaction mechanism? 1^st step: A ⇌ B very fast 2^nd step: B + C → D slow 3^rd step: D → 2E fast

What is a catalyst and what function does it serve?

Give the characteristic of a second order reaction having only one reactant.

Write a balanced reaction for which the following rate relationships are TRUE. Rate = = = -

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

The first-order decomposition of ammonium nitrate has a rate constant of 0.110 min^-1.If the initial concentration is 0.551 M,what is the concentration after 38.5 min?

In the hydrogenation of double bonds,a catalyst is needed.In the first step,the reactants must come into contact with a metal surface.This step is known as

Define activation energy.

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

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

The elementary reaction (g) → 2NO(g) + (g) is second order in and the rate constant at 501 K is 7.93 × 10^-3 .The reaction half-life at this temperature when = 0.45 M is ________ s.

Give the characteristic of a zero order reaction having only one reactant.

The combustion of ethylene proceeds by the reaction C₂H₄(g) + 3O₂(g) →2CO₂(g) + 2H₂O(g) When the rate of disappearance of O₂ is 0.28 M s^-1,the rate of appearance of CO₂ is ________ M s^-1.

Exam 15: Chemical Kinetics

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

What is the overall order of the following reaction,given the rate law? 2 X + 3 Y → 2 Z Rate = k[X]1[Y]2

For a certain reaction,a plot of ln [A] vs.time gives a straight line with a slope of -1.46 s-1 and a y-intercept of 4.30.What is the order of the reaction?

Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g) + O2(g) → 2 NO2(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

The rate constant for a second-order reaction is 0.54 M-1s-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

The rate constant for a first-order reaction is 0.54 s-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

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 M,what is the concentration of N2O5 after 12.5 minutes?

A reaction occurs via the following sequence of elementary steps.What is the rate law based on this reaction mechanism? 1st step: A ⇌ B very fast 2nd step: B + C → D slow 3rd step: D → 2E fast

What is a catalyst and what function does it serve?

Give the characteristic of a second order reaction having only one reactant.

Write a balanced reaction for which the following rate relationships are TRUE. Rate = = = -

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

The first-order decomposition of ammonium nitrate has a rate constant of 0.110 min-1.If the initial concentration is 0.551 M,what is the concentration after 38.5 min?

In the hydrogenation of double bonds,a catalyst is needed.In the first step,the reactants must come into contact with a metal surface.This step is known as

Define activation energy.

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

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

The elementary reaction (g) → 2NO(g) + (g) is second order in and the rate constant at 501 K is 7.93 × 10-3 .The reaction half-life at this temperature when = 0.45 M is ________ s.

Give the characteristic of a zero order reaction having only one reactant.

The combustion of ethylene proceeds by the reaction C2H4(g) + 3O2(g) →2CO2(g) + 2H2O(g) When the rate of disappearance of O2 is 0.28 M s-1,the rate of appearance of CO2 is ________ M s-1.

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

What is the overall order of the following reaction,given the rate law? 2 X + 3 Y → 2 Z Rate = k[X]¹[Y]²

For a certain reaction,a plot of ln [A] vs.time gives a straight line with a slope of -1.46 s^-1 and a y-intercept of 4.30.What is the order of the reaction?

Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g) + O₂(g) → 2 NO₂(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

The rate constant for a second-order reaction is 0.54 M^-1s^-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

The rate constant for a first-order reaction is 0.54 s^-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

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 M,what is the concentration of N₂O₅ after 12.5 minutes?

A reaction occurs via the following sequence of elementary steps.What is the rate law based on this reaction mechanism? 1^st step: A ⇌ B very fast 2^nd step: B + C → D slow 3^rd step: D → 2E fast

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

The first-order decomposition of ammonium nitrate has a rate constant of 0.110 min^-1.If the initial concentration is 0.551 M,what is the concentration after 38.5 min?

The elementary reaction (g) → 2NO(g) + (g) is second order in and the rate constant at 501 K is 7.93 × 10^-3 .The reaction half-life at this temperature when = 0.45 M is ________ s.

The combustion of ethylene proceeds by the reaction C₂H₄(g) + 3O₂(g) →2CO₂(g) + 2H₂O(g) When the rate of disappearance of O₂ is 0.28 M s^-1,the rate of appearance of CO₂ is ________ M s^-1.