Question 1

At elevated temperatures, nitrogen dioxide decomposes to nitrogen oxide and oxygen: NO2 (g) → NO (g) + 2 (g) → NO (g) +   O2 (g)  The reaction is second order in NO2 with a rate constant of 0.543 M-1s-1 at 300 °C. If the initial [NO2] is 0.260 M, it will take __________ s for the concentration to drop to 0.150 M. A) 3.34 B) 0.0880 C) 1.01 D) 0.299 E) 5.19" class="answers-bank-image d-inline" rel="preload" > O2 (g) 
The reaction is second order in NO2 with a rate constant of 0.543 M-1s-1 at 300 °C. If the initial [NO2] is 0.260 M, it will take __________ s for the concentration to drop to 0.150 M.

Accepted Answer

A)  3.34
B)  0.0880
C)  1.01
D)  0.299
E)  5.19F) B) and E)
G) A) and E)

Question 2

The earth's ozone layer is located in the __________.

Accepted Answer

The answer of The earth's ozone layer is located in...

Question 3

Of the following, __________ will lower the activation energy for a reaction.

Accepted Answer

A)  increasing the concentrations of reactants
B)  raising the temperature of the reaction
C)  adding a catalyst for the reaction
D)  removing products as the reaction proceeds
E)  increasing the pressureF) A) and D)
G) A) and E)

Question 4

The half-life for a first order rate law depends on the starting concentration.

Accepted Answer

A) True 
 B)False

Question 5

The rate law for this reaction is rate = __________.

Accepted Answer

A)  k[A][B]
B)  k[P]
C)  k[A]2[B]
D)  k[A]2[B]2
E)  k[A]2F) B) and E)
G) A) and E)

Question 6

A catalyst can increase the rate of a reaction __________.

Accepted Answer

A)  by changing the value of the frequency factor (
A)  
B)  by increasing the overall activation energy (Ea) of the reaction
C)  by lowering the activation energy of the reverse reaction
D)  by providing an alternative pathway with a lower activation energy
E)  All of these are ways that a catalyst might act to increase the rate of reaction.F) A) and E)
G) B) and E)

Question 7

If the rate law for the reaction 2A + 3B → products
Is first order in A and second order in B, then the rate law is rate = __________.

Accepted Answer

A)  k[A][B]
B)  k[A]2[B]3
C)  k[A][B]2
D)  k[A]2[B]
E)  k[A]2[B]2F) A) and B)
G) C) and D)

Question 8

The mechanism for formation of the product X is: A + B → C + D (slow) 
B + D → X (fast) 
The intermediate reactant in the reaction is __________.

Accepted Answer

A)  A
B)  B
C)  C
D)  D
E)  XF) B) and C)
G) A) and B)

Question 9

At elevated temperatures, methylisonitrile (CH3NC) isomerizes to acetonitrile (CH3CN) : CH3NC (g) → CH3CN (g) 
At the start of an experiment, there are 0.200 mol of reactant and 0 mol of product in the reaction vessel. After 25 min, 0.106 mol of reactant (CH3NC) remain. There are __________ mol of product (CH3CN) in the reaction vessel.

Accepted Answer

A)  0.022
B)  0.106
C)  0.200
D)  0.306
E)  0.094F) A) and E)
G) A) and D)

Question 10

The concentration of S2O82- remaining at 1600 s is __________ M.

Accepted Answer

A)  0.036
B)  0.014
C)  0.043
D)  0.064
E)  0.029F) B) and E)
G) D) and E)

Question 11

A catalyst that is present in a different phase from the reacting molecules is called a __________ catalyst.

Accepted Answer

The answer of A catalyst that is present in a...

Question 12

The rate constant for this reaction is __________ s-1.

Accepted Answer

A)  0.013
B)  0.030
C)  0.14
D)  3.0
E)  3.1 × 10-3F) C) and E)
G) A) and B)

Question 13

How many moles of B are present at 30 s?

Accepted Answer

A)  2.4 × 10-3
B)  0.15
C)  0.073
D)  1.7 × 10-3
E)  0.051F) B) and D)
G) A) and B)

Question 14

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

Accepted Answer

A)  9.56 × 103
B)  2.85 × 104
C)  576
D)  4.33 × 1087
E)  1.36 × 102F) B) and C)
G) A) and E)

Question 15

A particular first-order reaction has a rate constant of 1.35 × 102s-1 at 25.0°C. What is the magnitude of k at 75.0°C if Ea = 85.6 kJ/mol?

Accepted Answer

A)  3.47 × 104
B)  1.92 × 104
C)  670
D)  3.85 × 106
E)  1.36 × 102F) C) and D)
G) A) and B)

Question 16

The relationship of absorbed light to the concentration of the substance absorbing the light is governed by __________.

Accepted Answer

The answer of The relationship of absorbed light to the...

Question 17

The overall reaction order is the sum of the orders of each reactant in the rate law.

Accepted Answer

A) True 
 B)False

Question 18

The concentration of reactants or products at any time during the reaction can be calculated from the integrated rate law.

Accepted Answer

A) True 
 B)False

Question 19

The binding of molecules to the surface of a catalyst is referred to as __________.

Accepted Answer

The answer of The binding of molecules to the surface...

Question 20

The reaction A (aq) → B (aq) is first order in [A]. A solution is prepared with [A] = 1.22 M. The following data are obtained as the reaction proceeds: -1. A) 0.23 B) 1.0 C) 0.17 D) 0.12 E) -0.12" class="answers-bank-image d-inline" rel="preload" > The rate constant for this reaction is __________ s-1.

Accepted Answer

A)  0.23
B)  1.0
C)  0.17
D)  0.12
E)  -0.12F) None of the above
G) D) and E)

Exam 14: Chemical Kinetics

The binding of molecules to the surface of a catalyst is referred to as __________.

Correct Answer
verified

A catalyst can increase the rate of a reaction __________.

Correct Answer
verified

The half-life for a first order rate law depends on the starting concentration.

Correct Answer
verified

The reaction A (aq) → B (aq) is first order in [A]. A solution is prepared with [A] = 1.22 M. The following data are obtained as the reaction proceeds: The rate constant for this reaction is __________ s^-¹.

Correct Answer
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The concentration of S₂O₈^2- remaining at 1600 s is __________ M.

Correct Answer
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The rate law for this reaction is rate = __________.

Correct Answer
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The earth's ozone layer is located in the __________.

Correct Answer
verified

Of the following, __________ will lower the activation energy for a reaction.

Correct Answer
verified

The mechanism for formation of the product X is: A + B → C + D (slow) B + D → X (fast) The intermediate reactant in the reaction is __________.

Correct Answer
verified

How many moles of B are present at 30 s?

Correct Answer
verified

The rate constant for this reaction is __________ s^-1.

Correct Answer
verified

The relationship of absorbed light to the concentration of the substance absorbing the light is governed by __________.

Correct Answer
verified

If the rate law for the reaction 2A + 3B → products Is first order in A and second order in B, then the rate law is rate = __________.

Correct Answer
verified

The overall reaction order is the sum of the orders of each reactant in the rate law.

Correct Answer
verified

Correct Answer
verified

A particular first-order reaction has a rate constant of 1.35 × 10²s^-1 at 25.0°C. What is the magnitude of k at 75.0°C if E_a = 85.6 kJ/mol?

Correct Answer
verified

A catalyst that is present in a different phase from the reacting molecules is called a __________ catalyst.

Correct Answer
verified

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

Correct Answer
verified

The concentration of reactants or products at any time during the reaction can be calculated from the integrated rate law.

Correct Answer
verified

Correct Answer
verified

Exam 14: Chemical Kinetics

The binding of molecules to the surface of a catalyst is referred to as __________.

Correct AnswerverifiedShow Answer

A catalyst can increase the rate of a reaction __________.

Correct AnswerverifiedShow Answer

The half-life for a first order rate law depends on the starting concentration.

Correct AnswerverifiedShow Answer

The reaction A (aq) → B (aq) is first order in [A]. A solution is prepared with [A] = 1.22 M. The following data are obtained as the reaction proceeds: The rate constant for this reaction is __________ s-1.

Correct AnswerverifiedShow Answer

The concentration of S2O82- remaining at 1600 s is __________ M.

Correct AnswerverifiedShow Answer

The rate law for this reaction is rate = __________.

Correct AnswerverifiedShow Answer

The earth's ozone layer is located in the __________.

Correct AnswerverifiedShow Answer

Of the following, __________ will lower the activation energy for a reaction.

Correct AnswerverifiedShow Answer

The mechanism for formation of the product X is: A + B → C + D (slow) B + D → X (fast) The intermediate reactant in the reaction is __________.

Correct AnswerverifiedShow Answer

How many moles of B are present at 30 s?

Correct AnswerverifiedShow Answer

The rate constant for this reaction is __________ s-1.

Correct AnswerverifiedShow Answer

The relationship of absorbed light to the concentration of the substance absorbing the light is governed by __________.

Correct AnswerverifiedShow Answer

If the rate law for the reaction 2A + 3B → products Is first order in A and second order in B, then the rate law is rate = __________.

Correct AnswerverifiedShow Answer

The overall reaction order is the sum of the orders of each reactant in the rate law.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A particular first-order reaction has a rate constant of 1.35 × 102s-1 at 25.0°C. What is the magnitude of k at 75.0°C if Ea = 85.6 kJ/mol?

Correct AnswerverifiedShow Answer

A catalyst that is present in a different phase from the reacting molecules is called a __________ catalyst.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

The concentration of reactants or products at any time during the reaction can be calculated from the integrated rate law.

Correct AnswerverifiedShow Answer

At elevated temperatures, nitrogen dioxide decomposes to nitrogen oxide and oxygen: NO2 (g) → NO (g) + O2 (g) The reaction is second order in NO2 with a rate constant of 0.543 M-1s-1 at 300 °C. If the initial [NO2] is 0.260 M, it will take __________ s for the concentration to drop to 0.150 M.

Correct AnswerverifiedShow Answer

Correct Answer
verified

Correct Answer
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Correct Answer
verified

The reaction A (aq) → B (aq) is first order in [A]. A solution is prepared with [A] = 1.22 M. The following data are obtained as the reaction proceeds: The rate constant for this reaction is __________ s^-¹.

Correct Answer
verified

The concentration of S₂O₈^2- remaining at 1600 s is __________ M.

Correct Answer
verified

Correct Answer
verified

Correct Answer
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Correct Answer
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Correct Answer
verified

Correct Answer
verified

The rate constant for this reaction is __________ s^-1.

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
verified

A particular first-order reaction has a rate constant of 1.35 × 10²s^-1 at 25.0°C. What is the magnitude of k at 75.0°C if E_a = 85.6 kJ/mol?

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified