Question 1

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

Question 2

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 3

A particular first-order reaction has a rate constant of 1.35 × 3 s-1 B)  2.85 × 104 s-1 C)  576 s-1 D)  4.33 × 1087 s-1 E)  1.36 ×   s-1" class="answers-bank-image d-inline" rel="preload" > 3 s-1 B)  2.85 × 104 s-1 C)  576 s-1 D)  4.33 × 1087 s-1 E)  1.36 ×   s-1" class="answers-bank-image d-inline" rel="preload" > at 25.0°C.What is the magnitude of k at 3 s-1 B)  2.85 × 104 s-1 C)  576 s-1 D)  4.33 × 1087 s-1 E)  1.36 ×   s-1" class="answers-bank-image d-inline" rel="preload" >

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 × 3 s-1 
B)   2.85 × 104 s-1 
C)   576 s-1 
D)   4.33 × 1087 s-1 
E)   1.36 ×   s-1" class="answers-bank-image d-inline" rel="preload" > s-1

Question 4

The elementary reaction -3     .The reaction half-life at this temperature when   = 0.45 M is ________ s. A)  3.6 × 10-3 B)  0.011 C)  126 D)  87 E)  280" class="answers-bank-image d-inline" rel="preload" > (g) → 2NO(g) + -3     .The reaction half-life at this temperature when   = 0.45 M is ________ s. A)  3.6 × 10-3 B)  0.011 C)  126 D)  87 E)  280" class="answers-bank-image d-inline" rel="preload" > (g)  is second order in -3     .The reaction half-life at this temperature when   = 0.45 M is ________ s. A)  3.6 × 10-3 B)  0.011 C)  126 D)  87 E)  280" class="answers-bank-image d-inline" rel="preload" > and the rate constant at 501 K is 7.93 × 10-3 -3     .The reaction half-life at this temperature when   = 0.45 M is ________ s. A)  3.6 × 10-3 B)  0.011 C)  126 D)  87 E)  280" class="answers-bank-image d-inline" rel="preload" > -3     .The reaction half-life at this temperature when   = 0.45 M is ________ s. A)  3.6 × 10-3 B)  0.011 C)  126 D)  87 E)  280" class="answers-bank-image d-inline" rel="preload" > .The reaction half-life at this temperature when -3     .The reaction half-life at this temperature when   = 0.45 M is ________ s. A)  3.6 × 10-3 B)  0.011 C)  126 D)  87 E)  280" class="answers-bank-image d-inline" rel="preload" > = 0.45 M is ________ s.

Accepted Answer

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

Question 5

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 6

What is a catalyst and what function does it serve?

Accepted Answer

A catalyst is a substance that is not us...

Question 7

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 8

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 9

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 10

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 11

Define activation energy.

Accepted Answer

The activation energy is an en...

Question 12

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 13

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 14

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 15

Write a balanced reaction for which the following rate relationships are TRUE. Rate = 2 + O2 →      N2O B)  2 N2O → 2 N2 + O2 C)  N2O → N2 + 2 O2 D)    N2O →   N2 + O2 E)  2 N2 + O2 → 2 N2O" class="answers-bank-image d-inline" rel="preload" > 2 + O2 →      N2O B)  2 N2O → 2 N2 + O2 C)  N2O → N2 + 2 O2 D)    N2O →   N2 + O2 E)  2 N2 + O2 → 2 N2O" class="answers-bank-image d-inline" rel="preload" > = 2 + O2 →      N2O B)  2 N2O → 2 N2 + O2 C)  N2O → N2 + 2 O2 D)    N2O →   N2 + O2 E)  2 N2 + O2 → 2 N2O" class="answers-bank-image d-inline" rel="preload" > = - 2 + O2 →      N2O B)  2 N2O → 2 N2 + O2 C)  N2O → N2 + 2 O2 D)    N2O →   N2 + O2 E)  2 N2 + O2 → 2 N2O" class="answers-bank-image d-inline" rel="preload" > 2 + O2 →      N2O B)  2 N2O → 2 N2 + O2 C)  N2O → N2 + 2 O2 D)    N2O →   N2 + O2 E)  2 N2 + O2 → 2 N2O" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   2 + O2 →      N2O 
B)   2 N2O → 2 N2 + O2 
C)   N2O → N2 + 2 O2 
D)     N2O →   N2 + O2 
E)   2 N2 + O2 → 2 N2O" class="answers-bank-image d-inline" rel="preload" > N2 + O2 →    2 + O2 →      N2O 
B)   2 N2O → 2 N2 + O2 
C)   N2O → N2 + 2 O2 
D)     N2O →   N2 + O2 
E)   2 N2 + O2 → 2 N2O" class="answers-bank-image d-inline" rel="preload" > N2O
B)   2 N2O → 2 N2 + O2
C)   N2O → N2 + 2 O2
D)   2 + O2 →      N2O 
B)   2 N2O → 2 N2 + O2 
C)   N2O → N2 + 2 O2 
D)     N2O →   N2 + O2 
E)   2 N2 + O2 → 2 N2O" class="answers-bank-image d-inline" rel="preload" > N2O → 2 + O2 →      N2O 
B)   2 N2O → 2 N2 + O2 
C)   N2O → N2 + 2 O2 
D)     N2O →   N2 + O2 
E)   2 N2 + O2 → 2 N2O" class="answers-bank-image d-inline" rel="preload" > N2 + O2
E)   2 N2 + O2 → 2 N2O

Question 16

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 17

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 18

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 19

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 20

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

Accepted Answer

A)   t - [A]o = - kt 
D)   k = Ae(-Ea/RT)  
E)     =     + lnA" class="answers-bank-image d-inline" rel="preload" > = - kt
B)   t - [A]o = - kt 
D)   k = Ae(-Ea/RT)  
E)     =     + lnA" class="answers-bank-image d-inline" rel="preload" > - t - [A]o = - kt 
D)   k = Ae(-Ea/RT)  
E)     =     + lnA" class="answers-bank-image d-inline" rel="preload" > = kt
C)   [A]t - [A]o = - kt
D)   k = Ae(-Ea/RT) 
E)   t - [A]o = - kt 
D)   k = Ae(-Ea/RT)  
E)     =     + lnA" class="answers-bank-image d-inline" rel="preload" > = t - [A]o = - kt 
D)   k = Ae(-Ea/RT)  
E)     =     + lnA" class="answers-bank-image d-inline" rel="preload" > t - [A]o = - kt 
D)   k = Ae(-Ea/RT)  
E)     =     + lnA" class="answers-bank-image d-inline" rel="preload" > + lnA

Exam 15: Chemical Kinetics

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

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Define activation energy.

Correct AnswerverifiedThe activation energy is an en...View AnswerShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

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

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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

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

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

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

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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?

Correct AnswerverifiedShow Answer

What is a catalyst and what function does it serve?

Correct AnswerverifiedA catalyst is a substance that is not us...View AnswerShow Answer

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

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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?

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

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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

Correct Answer
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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?

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

Correct Answer
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Correct Answer
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The activation energy is an en...
View Answer

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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?

Correct Answer
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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.

Correct Answer
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Correct Answer
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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

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

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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?

Correct Answer
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Correct Answer
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A catalyst is a substance that is not us...
View Answer

Correct Answer
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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?

Correct Answer
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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.

Correct Answer
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Correct Answer
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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?

Correct Answer
verified

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

Correct Answer
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