Question 1

For the reaction A + B + C → products,the following initial-rate data were obtained.
[A]0 (mol/L) 
[B]0 (mol/L) 
[C]0 (mol/L) 
Initial Rate (mol/(L ∙ s) ) 
0) 40
0) 40
0) 20
0) 0160
0) 20
0) 40
0) 40
0) 0080
0) 60
0) 10
0) 20
0) 0015
0) 20
0) 10
0) 20
0) 0005
0) 20
0) 20
0) 40
0) 0020
What are the reaction orders with respect to A,B,and C,respectively?

Accepted Answer

A)  0,1,1
B)  1,2,1
C)  1,1,1
D)  1,2,0
E)  0,2,1

Question 2

A chemical reaction that is first-order in X is observed to have a rate constant of 2.00 × 10-2 s-1.If the initial concentration of X is 1.0 M,what is the concentration of X after 196 s?

Accepted Answer

A)  0.20 M
B)  0.020 M
C)  50 M
D)  0.61 M
E)  0.98 M

Question 3

A reaction that is second-order in one reactant has a rate constant of 3.8 × 10-2 L/(mol ∙ s) .If the initial concentration of the reactant is 0.280 mol/L,how long will it take for the concentration to become 0.140 mol/L?

Accepted Answer

A)  180 s
B)  47 s
C)  930 s
D)  18 s
E)  93 s

Question 4

The reaction
2H2(g) + 2NO(g) → 2H2O(g) + N2(g) 
Is first-order in H2 and second-order in NO at a particular temperature.What is the rate law?

Accepted Answer

A)  Rate = k[H2]2[NO]2
B)  Rate = k[H2][NO]2
C)  Rate = k[H2][NO]
D)  Rate = k[H2O]2[N2]
E)  Rate = k[H2]2[NO]

Question 5

For the first-order reaction
1/2 N2O4(g) → NO2(g) ; ΔH = 28.6 kJ
The activation energy is 53.7 kJ/mol.What is the activation energy for the reverse reaction?

Accepted Answer

A)  15.2 kJ/mol
B)  82.3 kJ/mol
C)  -53.7 kJ/mol
D)  25.1 kJ/mol
E)  53.7 kJ/mol

Question 6

Which of the following statements is incorrect?

Accepted Answer

A)  The rates of most chemical reactions change with time.
B)  The rate constant for a reaction can be changed by changing the temperature.
C)  The rate constant is dependent on the reactant concentrations.
D)  In a series of stepwise reactions,the rate-determining step is the slowest one.
E)  The rate of a catalyzed reaction is dependent on the concentration of the catalyst.

Question 7

For the hypothetical reaction A + 2B → 2C + D,the initial rate of disappearance of A is 2.0 × 10-2 mol/(L ∙ s) .What is the initial rate of disappearance of B?

Accepted Answer

A)  8.0 × 10-2 mol/(L ∙ s) 
B)  4 × 10-2 mol/(L ∙ s) 
C)  1.4 × 10-1 mol/(L ∙ s) 
D)  4.0 × 10-4 mol/(L ∙ s) 
E)  1.4 × 10-2 mol/(L ∙ s)

Question 8

For the elementary reaction A + B → C + D,what is the predicted rate law?

Accepted Answer

A)  Rate = k[A]2
B)  Rate = k[A][B]
C)  Rate = k 2 
B)  Rate = k[A][B] 
C)  Rate = k   
D)  Rate = k[B]2 
E)  Rate = k[A]/[C]" class="answers-bank-image d-inline" rel="preload" >
D)  Rate = k[B]2
E)  Rate = k[A]/[C]

Question 9

The catalyzed pathway in a reaction mechanism has a __________ activation energy and thus causes a __________ reaction rate.

Accepted Answer

A)  higher,lower
B)  higher,higher
C)  higher,steady
D)  lower,higher
E)  lower,steady

Question 10

The nuclide 188W decays by a first-order process with a rate constant of 1.0 × 10-2 d-1.How long will it take for 88% of the initial amount of 188W to be consumed?

Accepted Answer

A)  6 d
B)  240 d
C)  12 d
D)  210 d
E)  92 d

Question 11

Which of the following statements is incorrect?

Accepted Answer

A)  The slow step in a mechanism generally involves a three-body collision.
B)  After the addition of a catalyst,the collision rate between molecules is still the same.
C)  Most collisions between reactant molecules do not lead to a product.
D)  Chemical reactions involve collisions between the participating molecules.
E)  A three-body collision is less likely than a two-body collision.

Question 12

If a reaction is zero-order in a reactant,when the concentration of the reactant is decreased by a factor of 2,the reaction rate will

Accepted Answer

A)  quadruple.
B)  decrease by a factor of 1/2.
C)  remain constant.
D)  decrease by a factor of 1/4.
E)  double.

Question 13

For a certain reaction of the general form aA → products,a plot of the experimental data as [A] versus time is linear.What is the reaction order with respect to reactant A?

Accepted Answer

A)  zero
B)  first
C)  second
D)  fourth
E)  third

Question 14

At 500oC,cyclopropane (C3H6) reacts to form its isomer,propene (C3H6) .The reaction is first-order,and the rate constant is 6.7 × 10-4 s-1.If the initial concentration of cyclopropane is 0.500 M and the initial concentration of propene is 0,determine the time required for the concentration of propene to reach 0.100 M.

Accepted Answer

A)  3.4 × 103 s
B)  3.3 × 102 s
C)  1.2 × 104 s
D)  7.5 × 102 s
E)  2.4 × 103 s

Question 15

The reaction between selenous acid and the iodide ion in acid solution is
H2SeO3(aq) + 6I-(aq) + 4H+(aq) → Se(s) + 2I3-(aq) + 3H2O(l) 
The data in the following table were measured at 0°C.
Experiment
[H2SeO3]0 (M) 
[H+]0 (M) 
[I-]0 (M) 
Initial Rate [mol/(L ∙ s) ]
1
1) 00 × 10-4
2) 00 × 10-2
3) 00 × 10-2
5) 30 × 10-7
2
2) 00 × 10-4
2) 00 × 10-2
3) 00 × 10-2
1) 06 × 10-6
3
3) 00 × 10-4
4) 00 × 10-2
3) 00 × 10-2
6) 36 × 10-6
4
3) 00 × 10-4
8) 00 × 10-2
3) 00 × 10-2
2) 54 × 10-5
5
3) 00 × 10-4
8) 00 × 10-2
6) 00 × 10-2
2) 04 × 10-4
6
2) 00 × 10-4
2) 00 × 10-2
6) 00 × 10-2
8) 48 × 10-6
Tripling the initial concentration of H2SeO3 while holding the initial concentrations of H+ and I- constant increases the rate of the reaction by a factor of

Accepted Answer

A)  8.
B)  4.
C)  3.
D)  2.
E)  1.

Question 16

Nitrosyl chloride is produced from the reaction of nitrogen monoxide and chlorine:
2NO(g) + Cl2(g) → 2NOCl(g) 
The following initial rates at a given temperature were obtained for the concentrations listed below.
Experiment
Initial Rate (mol·L-1·h-1) 
[NO]0 (mol·L-1) 
[Cl2]0 (mol·L-1) 
1
2) 21
0) 25
0) 25
2
19) 89
0) 75
0) 25
3
6) 63
0) 25
0) 75
From the data,what is the experimental rate law?

Accepted Answer

A)  Rate = k[Cl2]
B)  Rate = k[NO]
C)  Rate = k[NO][Cl2]2
D)  Rate = k[NO]2[Cl2]
E)  Rate = k[NO][Cl2]1/2

Question 17

For the hypothetical first-order reaction A → products,k = 0.0822 s-1.If the initial concentration of A is 0.372 M,how long would it take for A to be 28.2% consumed?

Accepted Answer

A)  8.43 s
B)  4.03 s
C)  12 s
D)  32.7 s
E)  15.3 s

Question 18

The reaction between selenous acid and the iodide ion in acid solution is
H2SeO3(aq) + 6I-(aq) + 4H+(aq) → Se(s) + 2I3-(aq) + 3H2O(l) 
The data in the following table were measured at 0°C.
Experiment
[H2SeO3]0 (M) 
[H+]0 (M) 
[I-]0 (M) 
Initial Rate [mol/(L ∙ s) ]
1
1) 00 × 10-4
2) 00 × 10-2
3) 00 × 10-2
5) 30 × 10-7
2
2) 00 × 10-4
2) 00 × 10-2
3) 00 × 10-2
1) 06 × 10-6
3
3) 00 × 10-4
4) 00 × 10-2
3) 00 × 10-2
6) 36 × 10-6
4
3) 00 × 10-4
8) 00 × 10-2
3) 00 × 10-2
2) 54 × 10-5
5
3) 00 × 10-4
8) 00 × 10-2
6) 00 × 10-2
2) 04 × 10-4
6
2) 00 × 10-4
2) 00 × 10-2
6) 00 × 10-2
8) 48 × 10-6
The overall order of this reaction is

Accepted Answer

A)  4.
B)  6.
C)  2.
D)  8.
E)  3.

Question 19

A suggested mechanism for the decomposition of ozone is
O3 3   O2 + O fast equilibrium O + O3   2O2  slow step When the concentration of ozone is doubled and the concentration of oxygen is doubled,the instantaneous rate A) increases by a factor of 8. B) remains the same. C) increases by a factor of 4. D) decreases. E) increases by a factor of 2." class="answers-bank-image d-inline" rel="preload" >
O2 + O fast equilibrium
O + O3 3   O2 + O fast equilibrium O + O3   2O2  slow step When the concentration of ozone is doubled and the concentration of oxygen is doubled,the instantaneous rate A) increases by a factor of 8. B) remains the same. C) increases by a factor of 4. D) decreases. E) increases by a factor of 2." class="answers-bank-image d-inline" rel="preload" >
2O2  slow step
When the concentration of ozone is doubled and the concentration of oxygen is doubled,the instantaneous rate

Accepted Answer

A)  increases by a factor of 8.
B)  remains the same.
C)  increases by a factor of 4.
D)  decreases.
E)  increases by a factor of 2.

Question 20

The hypochlorite ion oxidizes the iodide ion in aqueous solution as represented by the following equation:
OCl-(aq) + I-(aq) → OI-(aq) + Cl-(aq) 
The rate law for this reaction is Rate = k -(aq) + I-(aq) → OI-(aq) + Cl-(aq)  The rate law for this reaction is Rate = k   ) The overall reaction order and the order with respect to OH- are A) 2 and -1. B) 0 and -1. C) 0 and 1. D) 2 and 1. E) 1 and -1." class="answers-bank-image d-inline" rel="preload" >
) The overall reaction order and the order with respect to OH- are

Accepted Answer

A)  2 and -1.
B)  0 and -1.
C)  0 and 1.
D)  2 and 1.
E)  1 and -1.

Exam 13: Rates of Reaction

Correct Answer
verified

For the hypothetical first-order reaction A → products,k = 0.0822 s^-1.If the initial concentration of A is 0.372 M,how long would it take for A to be 28.2% consumed?

Correct Answer
verified

Correct Answer
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For the hypothetical reaction A + 2B → 2C + D,the initial rate of disappearance of A is 2.0 × 10^-2 mol/(L ∙ s) .What is the initial rate of disappearance of B?

Correct Answer
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Which of the following statements is incorrect?

Correct Answer
verified

Which of the following statements is incorrect?

Correct Answer
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The hypochlorite ion oxidizes the iodide ion in aqueous solution as represented by the following equation: OCl^-(aq) + I^-(aq) → OI^-(aq) + Cl^-(aq) The rate law for this reaction is Rate = k ) The overall reaction order and the order with respect to OH^- are

Correct Answer
verified

A reaction that is second-order in one reactant has a rate constant of 3.8 × 10^-2 L/(mol ∙ s) .If the initial concentration of the reactant is 0.280 mol/L,how long will it take for the concentration to become 0.140 mol/L?

Correct Answer
verified

For a certain reaction of the general form aA → products,a plot of the experimental data as [A] versus time is linear.What is the reaction order with respect to reactant A?

Correct Answer
verified

Correct Answer
verified

The reaction 2H₂(g) + 2NO(g) → 2H₂O(g) + N₂(g) Is first-order in H₂ and second-order in NO at a particular temperature.What is the rate law?

Correct Answer
verified

For the elementary reaction A + B → C + D,what is the predicted rate law?

Correct Answer
verified

A chemical reaction that is first-order in X is observed to have a rate constant of 2.00 × 10^-2 s^-1.If the initial concentration of X is 1.0 M,what is the concentration of X after 196 s?

Correct Answer
verified

For the first-order reaction 1/2 N₂O₄(g) → NO₂(g) ; ΔH = 28.6 kJ The activation energy is 53.7 kJ/mol.What is the activation energy for the reverse reaction?

Correct Answer
verified

Correct Answer
verified

If a reaction is zero-order in a reactant,when the concentration of the reactant is decreased by a factor of 2,the reaction rate will

Correct Answer
verified

The nuclide ¹⁸⁸W decays by a first-order process with a rate constant of 1.0 × 10^-2 d^-1.How long will it take for 88% of the initial amount of ¹⁸⁸W to be consumed?

Correct Answer
verified

Correct Answer
verified

The catalyzed pathway in a reaction mechanism has a activation energy and thus causes a reaction rate.

Correct Answer
verified

A suggested mechanism for the decomposition of ozone is O₃ O₂ + O fast equilibrium O + O₃ 2O₂ slow step When the concentration of ozone is doubled and the concentration of oxygen is doubled,the instantaneous rate

Correct Answer
verified

Exam 13: Rates of Reaction

Correct AnswerverifiedShow Answer

For the hypothetical first-order reaction A → products,k = 0.0822 s-1.If the initial concentration of A is 0.372 M,how long would it take for A to be 28.2% consumed?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

For the hypothetical reaction A + 2B → 2C + D,the initial rate of disappearance of A is 2.0 × 10-2 mol/(L ∙ s) .What is the initial rate of disappearance of B?

Correct AnswerverifiedShow Answer

Which of the following statements is incorrect?

Correct AnswerverifiedShow Answer

Which of the following statements is incorrect?

Correct AnswerverifiedShow Answer

The hypochlorite ion oxidizes the iodide ion in aqueous solution as represented by the following equation: OCl-(aq) + I-(aq) → OI-(aq) + Cl-(aq) The rate law for this reaction is Rate = k ) The overall reaction order and the order with respect to OH- are

Correct AnswerverifiedShow Answer

A reaction that is second-order in one reactant has a rate constant of 3.8 × 10-2 L/(mol ∙ s) .If the initial concentration of the reactant is 0.280 mol/L,how long will it take for the concentration to become 0.140 mol/L?

Correct AnswerverifiedShow Answer

For a certain reaction of the general form aA → products,a plot of the experimental data as [A] versus time is linear.What is the reaction order with respect to reactant A?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The reaction 2H2(g) + 2NO(g) → 2H2O(g) + N2(g) Is first-order in H2 and second-order in NO at a particular temperature.What is the rate law?

Correct AnswerverifiedShow Answer

For the elementary reaction A + B → C + D,what is the predicted rate law?

Correct AnswerverifiedShow Answer

A chemical reaction that is first-order in X is observed to have a rate constant of 2.00 × 10-2 s-1.If the initial concentration of X is 1.0 M,what is the concentration of X after 196 s?

Correct AnswerverifiedShow Answer

For the first-order reaction 1/2 N2O4(g) → NO2(g) ; ΔH = 28.6 kJ The activation energy is 53.7 kJ/mol.What is the activation energy for the reverse reaction?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

If a reaction is zero-order in a reactant,when the concentration of the reactant is decreased by a factor of 2,the reaction rate will

Correct AnswerverifiedShow Answer

The nuclide 188W decays by a first-order process with a rate constant of 1.0 × 10-2 d-1.How long will it take for 88% of the initial amount of 188W to be consumed?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The catalyzed pathway in a reaction mechanism has a __________ activation energy and thus causes a __________ reaction rate.

Correct AnswerverifiedShow Answer

A suggested mechanism for the decomposition of ozone is O3 O2 + O fast equilibrium O + O3 2O2 slow step When the concentration of ozone is doubled and the concentration of oxygen is doubled,the instantaneous rate

Correct AnswerverifiedShow Answer

Correct Answer
verified

For the hypothetical first-order reaction A → products,k = 0.0822 s^-1.If the initial concentration of A is 0.372 M,how long would it take for A to be 28.2% consumed?

Correct Answer
verified

Correct Answer
verified

For the hypothetical reaction A + 2B → 2C + D,the initial rate of disappearance of A is 2.0 × 10^-2 mol/(L ∙ s) .What is the initial rate of disappearance of B?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The hypochlorite ion oxidizes the iodide ion in aqueous solution as represented by the following equation: OCl^-(aq) + I^-(aq) → OI^-(aq) + Cl^-(aq) The rate law for this reaction is Rate = k ) The overall reaction order and the order with respect to OH^- are

Correct Answer
verified

A reaction that is second-order in one reactant has a rate constant of 3.8 × 10^-2 L/(mol ∙ s) .If the initial concentration of the reactant is 0.280 mol/L,how long will it take for the concentration to become 0.140 mol/L?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The reaction 2H₂(g) + 2NO(g) → 2H₂O(g) + N₂(g) Is first-order in H₂ and second-order in NO at a particular temperature.What is the rate law?

Correct Answer
verified

Correct Answer
verified

A chemical reaction that is first-order in X is observed to have a rate constant of 2.00 × 10^-2 s^-1.If the initial concentration of X is 1.0 M,what is the concentration of X after 196 s?

Correct Answer
verified

For the first-order reaction 1/2 N₂O₄(g) → NO₂(g) ; ΔH = 28.6 kJ The activation energy is 53.7 kJ/mol.What is the activation energy for the reverse reaction?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The nuclide ¹⁸⁸W decays by a first-order process with a rate constant of 1.0 × 10^-2 d^-1.How long will it take for 88% of the initial amount of ¹⁸⁸W to be consumed?

Correct Answer
verified

Correct Answer
verified

The catalyzed pathway in a reaction mechanism has a activation energy and thus causes a reaction rate.

Correct Answer
verified

A suggested mechanism for the decomposition of ozone is O₃ O₂ + O fast equilibrium O + O₃ 2O₂ slow step When the concentration of ozone is doubled and the concentration of oxygen is doubled,the instantaneous rate

Correct Answer
verified