Question 1

For the reaction
2A + B $\rightarrow$ products
the following mechanism is proposed:
A + B  M
A + M $\rightarrow$ products
A catalyst never appears in a rate law.

Accepted Answer

A) True 
 B)False

Question 2

For the reaction
P4(g) + 5O2(g) $\rightarrow$ P4O10(s)
the following data were collected at a temperature for which Rate = -d[P4]/dt.  Determine the differential rate law and the value of the rate constant k.

Accepted Answer

Rate = k[P₄][O_...

Question 3

The activation energy for the reaction H2(g)  + I2(g)   →\rightarrow→ 2HI(g)  is changed from 184 kJ/mol to 59.0 kJ/mol at 600. K by the introduction of a Pt catalyst. Calculate the value of the ratio rate(catalyzed) /rate(uncatalyzed) .

Accepted Answer

A)   1.00
B)   0.321
C)   1.38
D)   7.62 *1010
E)   none of these

Question 4

A reaction represented by the equation
3OS1U1B12S1U1B0(g) $\rightarrow$2OS1U1B13S1U1B0(g)
was studied at a specific temperature, and the following data were collected. 
-Which is the value of the rate constant?

Accepted Answer

k = 3.47 * 10<sup>-<...

Question 5

The hypothetical reaction
2A $\rightarrow$ 2B + D
is assumed to have the mechanism   Derive the differential rate law for the production of D using the steady-state approximation.

Accepted Answer

The answer of The hypothetical reaction
2A $\rightarrow$ 2B + D
is...

Question 6

The decomposition of N2O5(g)  to NO2(g)  and O2(g)  obeys first-order kinetics. Assume the form of the rate law is
Rate 2O5(g)  to NO2(g)  and O2(g)  obeys first-order kinetics. Assume the form of the rate law is Rate   where k = 3.4 *10-5 s-1 at 25°C. -What is the initial rate of reaction at 25°C where [N2O5]0 = 5.0 *10-2 M? A)  3.4 * 10-5 mol/L • s B)  5.0 * 10-2 mol/L • s C)  6.8*10-4 mol/L • s D)  1.7* 10-6 mol/L • s E)  none of these " class="answers-bank-image d-inline" rel="preload" > where k = 3.4 *10-5 s-1 at 25°C.
-What is the initial rate of reaction at 25°C where [N2O5]0 = 5.0 *10-2 M?

Accepted Answer

A)   3.4 * 10-5 mol/L • s
B)   5.0 * 10-2 mol/L • s
C)   6.8*10-4 mol/L • s
D)   1.7* 10-6 mol/L • s
E)   none of these

Question 7

At a particular temperature, the half-life of a zero-order reaction is 21.0 min. How long will it take for the reactant concentration to be depleted by a factor of 8?

Accepted Answer

A)   63.0 min
B)   42.0 min
C)   36.8 min
D)   168 min
E)   147 min

Question 8

The following questions refer to the gas-phase decomposition of chloroethane:
C2H5Cl  →\rightarrow→ products
Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. 2H5Cl  \rightarrow products Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction.   -What was the initial concentration of the ethylene chloride? A)  0.02 M B)  0.22 M C)  0.35 M D)  0.29 M E)  0.11 M  " class="answers-bank-image d-inline" rel="preload" >
-What was the initial concentration of the ethylene chloride?

Accepted Answer

A)   0.02 M
B)   0.22 M
C)   0.35 M
D)   0.29 M
E)   0.11 M

Question 9

For a reaction aA  →\rightarrow→ products, [A]0 = 4.0 M, and the first three successive half-lives are 48, 96, and 192 min.
-Calculate k (without units) .

Accepted Answer

A)   5.2 * 10-3
B)   1.4 * 10-2
C)   2.6*10-3
D)   4.1*10-3
E)   none of these

Question 10

A general reaction written as 2A + 2B  C + 2D is studied and yields the following data.  C + 2D is studied and yields the following data.   -For the first of the reactions in the table of data, determine -[B]/t. A)  8.00  10-5 B)  1.60  10-4 C)  4.00  10-5 D)  2.00  10-5 E)  none of these " class="answers-bank-image d-inline" rel="preload" >
-For the first of the reactions in the table of data, determine -[B]/t.

Accepted Answer

A)   8.00  10-5
B)   1.60  10-4
C)   4.00  10-5
D)   2.00  10-5
E)   none of these

Question 11

For the reaction 2N2O5(g)   →\rightarrow→  4NO2(g)  + O2(g) , the following data were collected. 2O5(g)   \rightarrow  4NO2(g)  + O2(g) , the following data were collected.   -The concentration N2O5 at 100 min will be approximately A)  0.10*10-2 mol/L B)  0.01 *10-2 mol/L C)  0.06 * 10-2 mol/L D)  0.03 *10-2 mol/L E)  none of these  " class="answers-bank-image d-inline" rel="preload" >
-The concentration N2O5 at 100 min will be approximately

Accepted Answer

A)   0.10*10-2 mol/L
B)   0.01 *10-2 mol/L
C)   0.06 * 10-2 mol/L
D)   0.03 *10-2 mol/L
E)   none of these

Question 12

The following data were collected for the decay of HO2 radicals. 2 radicals.   Which of the following statements is true? A)  The half-life of the reaction is 2 ms. B)  A plot of 1/[HO2] versus time gives a straight line. C)  The rate of the reaction increases with time. D)  The decay of HO2 occurs by a first-order process. E)  A plot of ln [HO2] versus time is linear with a slope of -k. " class="answers-bank-image d-inline" rel="preload" > Which of the following statements is true?

Accepted Answer

A)   The half-life of the reaction is 2 ms.
B)   A plot of 1/[HO2] versus time gives a straight line.
C)   The rate of the reaction increases with time.
D)   The decay of HO2 occurs by a first-order process.
E)   A plot of ln [HO2] versus time is linear with a slope of -k.

Question 13

The reaction 2A + B  →\rightarrow→  C
Has the following proposed mechanism.
Step 1: A + B 2[B] B)  k[A]2[B]2 C)  k[A] D)  k[A][B] E)  k[A][B]2  " class="answers-bank-image d-inline" rel="preload" > D (fast equilibrium) 
Step 2: D + B  →\rightarrow→ E
Step 3: E + A →\rightarrow→ C + B
If step 2 is the rate-determining step, what should be the rate of formation of C?

Accepted Answer

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

Question 14

How many seconds would it take for the total pressure to be 0.7133 atm?

Accepted Answer

The answer of How many seconds would it take for...

Question 15

For a reaction aA  →\rightarrow→ products, [A]0 = 4.0 M, and the first three successive half-lives are 48, 96, and 192 min.
-The reaction A →\rightarrow→  B + C is known to be zero order in A with a rate constant of 4.2 *10-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]0 = 1.8 M. What is the concentration of B after 5.4 s?

Accepted Answer

A)   1.6 M
B)   5.2 * 10-1 M
C)   1.8 M
D)   2.3 *10-1 M
E)   1.0 * 10-1 M

Question 16

The reaction A  →\rightarrow→  B + C is known to be zero order in A with a rate constant of 3.8 *10-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]0 = 2.2 *10-3 M. What is the rate after 6.8 minutes?

Accepted Answer

A)   2.2 *10-3 mol/L • s
B)   3.8 * 10-2 mol/L • s
C)   8.4 *10-5 mol/L • s
D)   8.1 *10-4 mol/L • s
E)   1.5 *10-11 mol/L • s

Question 17

For the reaction 2N2O5(g)   →\rightarrow→  4NO2(g)  + O2(g) , the following data were collected. 2O5(g)   \rightarrow  4NO2(g)  + O2(g) , the following data were collected.   -The half-life of this reaction is approximately A)  18 min B)  36 min C)  15 min D)  23 min E)  45 min  " class="answers-bank-image d-inline" rel="preload" >
-The half-life of this reaction is approximately

Accepted Answer

A)   18 min
B)   36 min
C)   15 min
D)   23 min
E)   45 min

Question 18

The rate constant k is dependent on

Accepted Answer

A)   the concentration of the product.
B)   the order of the reaction.
C)   the temperature.
D)   the concentration of the reactant.
E)   none of these

Question 19

A general reaction written as 2A + 2B  C + 2D is studied and yields the following data.  C + 2D is studied and yields the following data.   -What is the order of the reaction with respect to A? A)  1 B)  0 C)  4 D)  3 E)  2 " class="answers-bank-image d-inline" rel="preload" >
-What is the order of the reaction with respect to A?

Accepted Answer

A)   1
B)   0
C)   4
D)   3
E)   2

Exam 15: Chemical Kinetics

How many seconds would it take for the total pressure to be 0.7133 atm?

Correct Answer
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Correct Answer
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Correct Answer
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The decomposition of N₂O₅(g) to NO₂(g) and O₂(g) obeys first-order kinetics. Assume the form of the rate law is Rate where k = 3.4 10^-⁵ s^-¹ at 25°C. -What is the initial rate of reaction at 25°C where [N₂O₅]₀ = 5.0 10^-² M?

Correct Answer
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The reaction A $\rightarrow$ B + C is known to be zero order in A with a rate constant of 3.8 10^-² mol/L • s at 25° C. An experiment was run at 25°C where [A]₀ = 2.2 10^-³ M. What is the rate after 6.8 minutes?

Correct Answer
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Correct Answer
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Correct Answer
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The following data were collected for the decay of HO₂ radicals. Which of the following statements is true?

Correct Answer
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A general reaction written as 2A + 2B  C + 2D is studied and yields the following data. -What is the order of the reaction with respect to A?

Correct Answer
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Correct Answer
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Correct Answer
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Rate = k[P₄][O_...
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A general reaction written as 2A + 2B  C + 2D is studied and yields the following data. -For the first of the reactions in the table of data, determine -[B]/t.

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Correct Answer
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Correct Answer
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Correct Answer
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k = 3.47 * 10^-<...
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For a reaction aA $\rightarrow$ products, [A]₀= 4.0 M, and the first three successive half-lives are 48, 96, and 192 min. -Calculate k (without units) .

Correct Answer
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The activation energy for the reaction H₂(g) + I₂(g) $\rightarrow$ 2HI(g) is changed from 184 kJ/mol to 59.0 kJ/mol at 600. K by the introduction of a Pt catalyst. Calculate the value of the ratio rate(catalyzed) /rate(uncatalyzed) .

Correct Answer
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The rate constant k is dependent on

Correct Answer
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At a particular temperature, the half-life of a zero-order reaction is 21.0 min. How long will it take for the reactant concentration to be depleted by a factor of 8?

Correct Answer
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Exam 15: Chemical Kinetics

How many seconds would it take for the total pressure to be 0.7133 atm?

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The reaction 2A + B →\rightarrow→ C Has the following proposed mechanism. Step 1: A + B D (fast equilibrium) Step 2: D + B →\rightarrow→ E Step 3: E + A →\rightarrow→ C + B If step 2 is the rate-determining step, what should be the rate of formation of C?

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For the reaction 2N2O5(g) →\rightarrow→ 4NO2(g) + O2(g) , the following data were collected. -The concentration N2O5 at 100 min will be approximately

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The decomposition of N2O5(g) to NO2(g) and O2(g) obeys first-order kinetics. Assume the form of the rate law is Rate where k = 3.4 *10-5 s-1 at 25°C. -What is the initial rate of reaction at 25°C where [N2O5]0 = 5.0 *10-2 M?

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The reaction A →\rightarrow→ B + C is known to be zero order in A with a rate constant of 3.8 *10-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]0 = 2.2 *10-3 M. What is the rate after 6.8 minutes?

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For the reaction 2N2O5(g) →\rightarrow→ 4NO2(g) + O2(g) , the following data were collected. -The half-life of this reaction is approximately

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The hypothetical reaction 2A →\rightarrow→ 2B + D is assumed to have the mechanism Derive the differential rate law for the production of D using the steady-state approximation.

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The following data were collected for the decay of HO2 radicals. Which of the following statements is true?

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A general reaction written as 2A + 2B  C + 2D is studied and yields the following data. -What is the order of the reaction with respect to A?

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For the reaction 2A + B →\rightarrow→ products the following mechanism is proposed: A + B M A + M →\rightarrow→ products A catalyst never appears in a rate law.

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For the reaction P4(g) + 5O2(g) →\rightarrow→ P4O10(s) the following data were collected at a temperature for which Rate = -d[P4]/dt. Determine the differential rate law and the value of the rate constant k.

Correct AnswerverifiedRate = k[P4][O...View AnswerShow Answer

A general reaction written as 2A + 2B  C + 2D is studied and yields the following data. -For the first of the reactions in the table of data, determine -[B]/t.

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The following questions refer to the gas-phase decomposition of chloroethane: C2H5Cl →\rightarrow→ products Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. -What was the initial concentration of the ethylene chloride?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A reaction represented by the equation 3O2(g) →\rightarrow→ 2O3(g) was studied at a specific temperature, and the following data were collected. -Which is the value of the rate constant?

Correct Answerverifiedk = 3.47 * 10-<...View AnswerShow Answer

For a reaction aA →\rightarrow→ products, [A]0 = 4.0 M, and the first three successive half-lives are 48, 96, and 192 min. -Calculate k (without units) .

Correct AnswerverifiedShow Answer

The activation energy for the reaction H2(g) + I2(g) →\rightarrow→ 2HI(g) is changed from 184 kJ/mol to 59.0 kJ/mol at 600. K by the introduction of a Pt catalyst. Calculate the value of the ratio rate(catalyzed) /rate(uncatalyzed) .

Correct AnswerverifiedShow Answer

The rate constant k is dependent on

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At a particular temperature, the half-life of a zero-order reaction is 21.0 min. How long will it take for the reactant concentration to be depleted by a factor of 8?

Correct AnswerverifiedShow Answer

Correct Answer
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Correct Answer
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Correct Answer
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The decomposition of N₂O₅(g) to NO₂(g) and O₂(g) obeys first-order kinetics. Assume the form of the rate law is Rate where k = 3.4 10^-⁵ s^-¹ at 25°C. -What is the initial rate of reaction at 25°C where [N₂O₅]₀ = 5.0 10^-² M?

Correct Answer
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The reaction A $\rightarrow$ B + C is known to be zero order in A with a rate constant of 3.8 10^-² mol/L • s at 25° C. An experiment was run at 25°C where [A]₀ = 2.2 10^-³ M. What is the rate after 6.8 minutes?

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Correct Answer
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Correct Answer
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The following data were collected for the decay of HO₂ radicals. Which of the following statements is true?

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Rate = k[P₄][O_...
View Answer

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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k = 3.47 * 10^-<...
View Answer

For a reaction aA $\rightarrow$ products, [A]₀= 4.0 M, and the first three successive half-lives are 48, 96, and 192 min. -Calculate k (without units) .

Correct Answer
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The activation energy for the reaction H₂(g) + I₂(g) $\rightarrow$ 2HI(g) is changed from 184 kJ/mol to 59.0 kJ/mol at 600. K by the introduction of a Pt catalyst. Calculate the value of the ratio rate(catalyzed) /rate(uncatalyzed) .

Correct Answer
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Correct Answer
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Correct Answer
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