Question 1

For the second-order reaction A → products,the following data are obtained:
[A] = 1.512 M,t = 0 min
[A] = 1.490 M,t = 1.0 min
[A] = 1.469 M,t = 2.0 min
What is the initial rate of the reaction in the experiment?

Accepted Answer

A)  0.40 M/min
B)  0.022 M/min
C)  0.089 M/min
D)  9.8 × 10-3 M/min
E)  0.046 M/minF) A) and E)
G) B) and D)

Question 2

Which of the following has no effect on the rate of a reaction?

Accepted Answer

A)  value of ΔH°
B)  activation energy
C)  presence of a catalyst
D)  temperature of reactants
E)  concentrations of reactantsF) C) and D)
G) A) and C)

Question 3

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00?

Accepted Answer

A)  The rate will decrease by a factor of 1/25.0.
B)  The rate will decrease by a factor of 1/5.00.
C)  The rate will increase by a factor of 5.00.
D)  The rate will increase by a factor of 25.0.E) B) and D)
F) None of the above

Question 4

5" class="answers-bank-image d-inline" rel="preload" > 5" class="answers-bank-image d-inline" rel="preload" > Decomposes in the gas phase by the reaction 5" class="answers-bank-image d-inline" rel="preload" >
The reaction is first order in 5" class="answers-bank-image d-inline" rel="preload" > 5" class="answers-bank-image d-inline" rel="preload" > And the rate constant is 3.0 × 5" class="answers-bank-image d-inline" rel="preload" > 5" class="answers-bank-image d-inline" rel="preload" > At 600 K.A vessel is charged with 2.4 atm of 5" class="answers-bank-image d-inline" rel="preload" > At 600 K.The partial pressure of 5" class="answers-bank-image d-inline" rel="preload" > 5" class="answers-bank-image d-inline" rel="preload" > At 5" class="answers-bank-image d-inline" rel="preload" > Is ________ atm.

Accepted Answer

A)  0.76
B)  2.2
C)  0.98
D)  0.29
E)  1.4 × 105F) None of the above
G) B) and C)

Question 5

Choose the INCORRECT answer.The rate of a chemical reaction:

Accepted Answer

A)  usually is increased when the concentration of one of the reactants is increased
B)  is dependent on temperature
C)  may be increased by certain catalytic agents
D)  will be very rapid if the activation energy is large
E)  describes the rate of change in concentration of a reactant or product with timeF) B) and D)
G) A) and C)

Question 6

In aqueous solution,hypobromite ion,BrO-,reacts to produce bromate ion,BrO3-,and bromide ion,Br-,according to the following chemical equation: 
-,reacts to produce bromate ion,BrO3-,and bromide ion,Br-,according to the following chemical equation:    A plot of 1/[BrO-] vs.time is linear and the slope is equal to 0.056 L mol-1 s-1.If the initial concentration of BrO- is 0.80 mol L-1,how long will it take one-half of the BrO- ion to react? A) 4.5 × 10-2 s B) 7.1 s C) 12 s D) 22 s" class="answers-bank-image d-inline" rel="preload" >
A plot of 1/[BrO-] vs.time is linear and the slope is equal to 0.056 L mol-1 s-1.If the initial concentration of BrO- is 0.80 mol L-1,how long will it take one-half of the BrO- ion to react?

Accepted Answer

A)  4.5 × 10-2 s
B)  7.1 s
C)  12 s
D)  22 sE) All of the above
F) C) and D)

Question 7

For the reaction: 2 N2O5(g) → 4 NO2(g) + O2(g) the rate law is: 
2O5(g) → 4 NO2(g) + O2(g) the rate law is:    = k[N2O5] At 300 K,the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol O2.What is the half-life at 350 K? A) 67.3 s B) 9.3 × 106 s C) 1.09 × 10-17 s D) 2.48 × 104 s E) 0.145 s" class="answers-bank-image d-inline" rel="preload" > = k[N2O5]
At 300 K,the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol O2.What is the half-life at 350 K?

Accepted Answer

A)  67.3 s
B)  9.3 × 106 s
C)  1.09 × 10-17 s
D)  2.48 × 104 s
E)  0.145 sF) A) and B)
G) None of the above

Question 8

If the half-life of a reactant is independent of its initial concentration,the reaction order is 0.

Accepted Answer

A) True 
 B)False

Question 9

If a catalyst is added to a reaction:
I.the value of k is increased
II.the value of k is decreased
III.the rate is increased
IV.the rate is decreased
V.neither rate nor the constant are changed,only the order

Accepted Answer

A)  I and IV
B)  II and IV
C)  II and III
D)  I and III
E)  V onlyF) B) and C)
G) C) and E)

Question 10

Which of the following is FALSE for a second order reaction?

Accepted Answer

A)  1/[A]t - 1/[A]o = kt.
B)  t1/2 = 1/k[A]o.
C)  If 1/[A] versus time is a straight line,the reaction is second order.
D)  Each successive half-life is 4 times as long as the previous.
E)  The slope of 1/[A]t versus time is k.F) A) and D)
G) A) and C)

Question 11

If increasing the concentration of A in a chemical reaction causes no increase in the rate of the reaction,then we may say the reaction rate is first order in [A].

Accepted Answer

A) True 
 B)False

Question 12

The isomerization reaction,CH3NC → CH3CN,is first order and the rate constant is equal to 0.46 s-1 at 600 K.What is the concentration of CH3NC after 0.20 minutes if the initial concentration is 0.30 mol L-1?

Accepted Answer

A)  1.2 × 10-3 mol L-1
B)  2.7 × 10-3 mol L-1
C)  1.2 × 10-1 mol L-1
D)  2.7 × 10-1 mol L-1E) A) and B)
F) B) and C)

Question 13

Nitrogen dioxide decomposes at 300 °C via a second-order process to produce nitrogen monoxide and oxygen according to the following chemical equation:
2 NO2(g) → 2 NO(g) + O2(g) .
A sample of NO2(g) is initially placed in a 2.50 L reaction vessel at 300 °C.If the half-life and the rate constant at 300 °C are 11 seconds and 0.54 L mol-1 s-1,respectively,how many moles of NO2 were in the original sample?

Accepted Answer

A)  0.17 mol
B)  0.42 mol
C)  5.9 mol
D)  15 molE) None of the above
F) All of the above

Question 14

Substance A decomposes by a first-order reaction.Starting initially with [A] = 2.00 M,after 150 min [A] = 0.50 M.For this reaction what is  ?

Accepted Answer

A)  150 min
B)  37.5 min
C)  75.0 min
D)  15.0 min
E)  300 minF) A) and B)
G) A) and C)

Question 15

For the reaction: 2 NO2(g) → 2 NO(g) + O2(g) concentration-time data are:
2(g) → 2 NO(g) + O2(g) concentration-time data are:   What is the order of the reaction with respect to [NO2]? A) zero B) first C) second D) third E) 2 + 2" class="answers-bank-image d-inline" rel="preload" >
What is the order of the reaction with respect to [NO2]?

Accepted Answer

A)  zero
B)  first
C)  second
D)  third
E)  2 + 2F) C) and E)
G) A) and B)

Question 16

Define rate law.

Accepted Answer

A)  A theoretical equation that describes how the rate of reaction depends on the concentration of reactants.
B)  An experimentally determined equation that describes how the rate of reaction depends on the concentration of reactants.
C)  A theoretical equation that describes how the rate of reaction depends on temperature,orientation and number of collisions.
D)  An experimentally determined equation that describes how the rate of reaction depends on temperature,orientation and number of collisions.
E)  A statement that describes how the ratio of reaction depends on concentration of reactants developed from the balanced equation.F) B) and C)
G) C) and D)

Question 17

For the first-order reaction,2 N2O(g) → 2 N2(g) + O2(g) ,what is the concentration of N2O after 3 half-lives if 2O(g) → 2 N2(g) + O2(g) ,what is the concentration of N2O after 3 half-lives if   Mol of N2O is initially placed into a 1.00 L reaction vessel? 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" class="answers-bank-image d-inline" rel="preload" > 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-1E) None of the above
F) B) and D)

Question 18

What is the rate constant at 305 K for the reaction:
2 N2O5 → 2 N2O4 + O2,
If k = 3.46 × 10-5 s-1 at 298 K and Ea = 106 kJ/mol?

Accepted Answer

A)  2.4 × 10-5 s-1 
B)  4.8 × 10-5 s-1 
C)  6.0 × 10-5 s-1 
D)  1.2 × 10-5 s-1 
E)  9.2 × 10-5 s-1 F) C) and D)
G) B) and D)

Question 19

Which of the following statements is true about the reaction 2 A → B + C which is first order in A and first order overall?

Accepted Answer

A)  The rate of the reaction will decrease at higher concentrations of B and C.
B)  The time required for one half of A to react is directly proportional to the quantity of A.
C)  The rate of formation of C is twice the rate of reaction of A.
D)  The rate of formation of B is the same as the rate of reaction of A.
E)  The initial rate doubles with doubling of initial concentration of A.F) C) and D)
G) B) and E)

Question 20

For 2 NO + O2 → 2 NO2,initial rate data are:
2 → 2 NO2,initial rate data are:   The rate law is Rate = k[NO][O2]y: A) x = 1,y = 2 B) x = 2,y = 1 C) x = 1,y = 1 D) x = 2,y = 2 E) x = 0,y = 2" class="answers-bank-image d-inline" rel="preload" >
The rate law is Rate = k[NO][O2]y:

Accepted Answer

A)  x = 1,y = 2
B)  x = 2,y = 1
C)  x = 1,y = 1
D)  x = 2,y = 2
E)  x = 0,y = 2F) B) and D)
G) A) and D)

Exam 20: Chemical Kinetics

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

Correct Answer
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Correct Answer
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What is the rate constant at 305 K for the reaction: 2 N₂O₅ → 2 N₂O₄ + O₂, If k = 3.46 × 10^-5 s^-1 at 298 K and E_a = 106 kJ/mol?

Correct Answer
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For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00?

Correct Answer
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For the reaction: 2 NO₂(g) → 2 NO(g) + O₂(g) concentration-time data are: What is the order of the reaction with respect to [NO₂]?

Correct Answer
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Substance A decomposes by a first-order reaction.Starting initially with [A] = 2.00 M,after 150 min [A] = 0.50 M.For this reaction what is ?

Correct Answer
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Define rate law.

Correct Answer
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Which of the following is FALSE for a second order reaction?

Correct Answer
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Choose the INCORRECT answer.The rate of a chemical reaction:

Correct Answer
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For the second-order reaction A → products,the following data are obtained: [A] = 1.512 M,t = 0 min [A] = 1.490 M,t = 1.0 min [A] = 1.469 M,t = 2.0 min What is the initial rate of the reaction in the experiment?

Correct Answer
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If a catalyst is added to a reaction: I.the value of k is increased II.the value of k is decreased III.the rate is increased IV.the rate is decreased V.neither rate nor the constant are changed,only the order

Correct Answer
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If increasing the concentration of A in a chemical reaction causes no increase in the rate of the reaction,then we may say the reaction rate is first order in [A].

Correct Answer
verified

Decomposes in the gas phase by the reaction The reaction is first order in And the rate constant is 3.0 × At 600 K.A vessel is charged with 2.4 atm of At 600 K.The partial pressure of At Is ________ atm.

Correct Answer
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If the half-life of a reactant is independent of its initial concentration,the reaction order is 0.

Correct Answer
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Which of the following has no effect on the rate of a reaction?

Correct Answer
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For the reaction: 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) the rate law is: = k[N₂O₅] At 300 K,the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol O₂.What is the half-life at 350 K?

Correct Answer
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The isomerization reaction,CH₃NC → CH₃CN,is first order and the rate constant is equal to 0.46 s^-1 at 600 K.What is the concentration of CH₃NC after 0.20 minutes if the initial concentration is 0.30 mol L^-1?

Correct Answer
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For 2 NO + O₂ → 2 NO₂,initial rate data are: The rate law is Rate = k[NO][O₂]^y:

Correct Answer
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Correct Answer
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Which of the following statements is true about the reaction 2 A → B + C which is first order in A and first order overall?

Correct Answer
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Exam 20: Chemical Kinetics

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

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

What is the rate constant at 305 K for the reaction: 2 N2O5 → 2 N2O4 + O2, If k = 3.46 × 10-5 s-1 at 298 K and Ea = 106 kJ/mol?

Correct AnswerverifiedShow Answer

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00?

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For the reaction: 2 NO2(g) → 2 NO(g) + O2(g) concentration-time data are: What is the order of the reaction with respect to [NO2]?

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Substance A decomposes by a first-order reaction.Starting initially with [A] = 2.00 M,after 150 min [A] = 0.50 M.For this reaction what is ?

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Define rate law.

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Which of the following is FALSE for a second order reaction?

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Choose the INCORRECT answer.The rate of a chemical reaction:

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For the second-order reaction A → products,the following data are obtained: [A] = 1.512 M,t = 0 min [A] = 1.490 M,t = 1.0 min [A] = 1.469 M,t = 2.0 min What is the initial rate of the reaction in the experiment?

Correct AnswerverifiedShow Answer

If a catalyst is added to a reaction: I.the value of k is increased II.the value of k is decreased III.the rate is increased IV.the rate is decreased V.neither rate nor the constant are changed,only the order

Correct AnswerverifiedShow Answer

If increasing the concentration of A in a chemical reaction causes no increase in the rate of the reaction,then we may say the reaction rate is first order in [A].

Correct AnswerverifiedShow Answer

Decomposes in the gas phase by the reaction The reaction is first order in And the rate constant is 3.0 × At 600 K.A vessel is charged with 2.4 atm of At 600 K.The partial pressure of At Is ________ atm.

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If the half-life of a reactant is independent of its initial concentration,the reaction order is 0.

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Which of the following has no effect on the rate of a reaction?

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For the reaction: 2 N2O5(g) → 4 NO2(g) + O2(g) the rate law is: = k[N2O5] At 300 K,the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol O2.What is the half-life at 350 K?

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The isomerization reaction,CH3NC → CH3CN,is first order and the rate constant is equal to 0.46 s-1 at 600 K.What is the concentration of CH3NC after 0.20 minutes if the initial concentration is 0.30 mol L-1?

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For 2 NO + O2 → 2 NO2,initial rate data are: The rate law is Rate = k[NO][O2]y:

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Correct AnswerverifiedShow Answer

Which of the following statements is true about the reaction 2 A → B + C which is first order in A and first order overall?

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

Correct Answer
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Correct Answer
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What is the rate constant at 305 K for the reaction: 2 N₂O₅ → 2 N₂O₄ + O₂, If k = 3.46 × 10^-5 s^-1 at 298 K and E_a = 106 kJ/mol?

Correct Answer
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For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00?

Correct Answer
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For the reaction: 2 NO₂(g) → 2 NO(g) + O₂(g) concentration-time data are: What is the order of the reaction with respect to [NO₂]?

Correct Answer
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Correct Answer
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For the reaction: 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) the rate law is: = k[N₂O₅] At 300 K,the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol O₂.What is the half-life at 350 K?

Correct Answer
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The isomerization reaction,CH₃NC → CH₃CN,is first order and the rate constant is equal to 0.46 s^-1 at 600 K.What is the concentration of CH₃NC after 0.20 minutes if the initial concentration is 0.30 mol L^-1?

Correct Answer
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For 2 NO + O₂ → 2 NO₂,initial rate data are: The rate law is Rate = k[NO][O₂]^y:

Correct Answer
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