Question 1

Which quantity is greatest?

Accepted Answer

A)   acivation energy of the reverse reaction
B)   absolute enthalpy of the reaction
C)   activation energy of the forward reactionD) B) and C)
E) A) and C)

Question 2

Tabulated below are initial rate data for the reaction
2Fe(CN) 63- + 2I- → 2Fe(CN) 64- + I2 63- + 2I- → 2Fe(CN) 64- + I2   What is the experimental rate law? A)    k[Fe(CN) 63-][I-]2 B)    k[Fe(CN) 63-][I-] [Fe(CN) 64-] C)    k[Fe(CN) 63-]2[I-] D)    k[Fe(CN) 63-]2[I-]2[Fe(CN) 64-]2[I2] E)    k[Fe(CN) 63-]2[I-][Fe(CN) 64-][I2]" class="answers-bank-image d-inline" rel="preload" >
What is the experimental rate law?

Accepted Answer

A)   63- + 2I- → 2Fe(CN) 64- + I2   What is the experimental rate law? 
A)     k[Fe(CN) 63-][I-]2 
B)     k[Fe(CN) 63-][I-] [Fe(CN) 64-] 
C)     k[Fe(CN) 63-]2[I-] 
D)     k[Fe(CN) 63-]2[I-]2[Fe(CN) 64-]2[I2] 
E)     k[Fe(CN) 63-]2[I-][Fe(CN) 64-][I2]" class="answers-bank-image d-inline" rel="preload" > k[Fe(CN) 63-][I-]2
B)   63- + 2I- → 2Fe(CN) 64- + I2   What is the experimental rate law? 
A)     k[Fe(CN) 63-][I-]2 
B)     k[Fe(CN) 63-][I-] [Fe(CN) 64-] 
C)     k[Fe(CN) 63-]2[I-] 
D)     k[Fe(CN) 63-]2[I-]2[Fe(CN) 64-]2[I2] 
E)     k[Fe(CN) 63-]2[I-][Fe(CN) 64-][I2]" class="answers-bank-image d-inline" rel="preload" > k[Fe(CN) 63-][I-] [Fe(CN) 64-]
C)   63- + 2I- → 2Fe(CN) 64- + I2   What is the experimental rate law? 
A)     k[Fe(CN) 63-][I-]2 
B)     k[Fe(CN) 63-][I-] [Fe(CN) 64-] 
C)     k[Fe(CN) 63-]2[I-] 
D)     k[Fe(CN) 63-]2[I-]2[Fe(CN) 64-]2[I2] 
E)     k[Fe(CN) 63-]2[I-][Fe(CN) 64-][I2]" class="answers-bank-image d-inline" rel="preload" > k[Fe(CN) 63-]2[I-]
D)   63- + 2I- → 2Fe(CN) 64- + I2   What is the experimental rate law? 
A)     k[Fe(CN) 63-][I-]2 
B)     k[Fe(CN) 63-][I-] [Fe(CN) 64-] 
C)     k[Fe(CN) 63-]2[I-] 
D)     k[Fe(CN) 63-]2[I-]2[Fe(CN) 64-]2[I2] 
E)     k[Fe(CN) 63-]2[I-][Fe(CN) 64-][I2]" class="answers-bank-image d-inline" rel="preload" > k[Fe(CN) 63-]2[I-]2[Fe(CN) 64-]2[I2]
E)   63- + 2I- → 2Fe(CN) 64- + I2   What is the experimental rate law? 
A)     k[Fe(CN) 63-][I-]2 
B)     k[Fe(CN) 63-][I-] [Fe(CN) 64-] 
C)     k[Fe(CN) 63-]2[I-] 
D)     k[Fe(CN) 63-]2[I-]2[Fe(CN) 64-]2[I2] 
E)     k[Fe(CN) 63-]2[I-][Fe(CN) 64-][I2]" class="answers-bank-image d-inline" rel="preload" > k[Fe(CN) 63-]2[I-][Fe(CN) 64-][I2]F) None of the above
G) B) and D)

Question 3

For the reaction
CH3CHCH2(g) + HCl(g) → CH3CHClCH3(g)
a possible mechanism is  
Fast equilibrium  
  
Fast equilibrium
Complex + (HCl)2  
CH3CHClCH3 + 2HCl
Slow
Derive the rate law for this reaction using this mechanism.

Accepted Answer

Question 4

The reaction
3NO → N2O + NO2
Is found to obey the rate law Rate = k[NO]2. If the first half-life of the reaction is found to be 3.5 s, what is the length of the fourth half-life?

Accepted Answer

A)   21 s
B)   6.6 s
C)   53 s
D)   14 s
E)   56 sF) D) and E)
G) A) and B)

Question 5

For the reaction 2N2O5(g)  → 4NO2(g)  + O2(g) , the following data were collected. 2O5(g)  → 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 minF) A) and B)
G) B) and C)

Question 6

Consider the second-order reaction aA → products (which has a first half-life of 25 s) . If the concentration of A after 15.6s is 0.36M, determine the initial concentration of A.

Accepted Answer

A)   0.58M
B)   0.26M
C)   0.53M
D)   0.14M
E)   0.16MF) A) and D)
G) A) and C)

Question 7

The following questions refer to the reaction 2A2 + B2 → 2C. The mechanism below has been proposed: 2 + B2 → 2C. The mechanism below has been proposed:   -The activation energy for the reaction H2(g)  + I2(g)  → 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) . A)  1.00 B)  0.321 C)  1.38 D)  7.62 × 1010 E)  none of these " class="answers-bank-image d-inline" rel="preload" >
-The activation energy for the reaction H2(g)  + I2(g)  → 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 theseF) B) and D)
G) A) and C)

Question 8

Use the potential energy diagram shown to answer the following questions. 
-Which letter shows the change in energy for the overall reaction?

Accepted Answer

The answer of Use the potential energy diagram shown to...

Question 9

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 10

A general reaction written as 2A + 2B → C + 2D is studied and yields the following data. -1 B)  4.00 × 10-2 C)  4.00 × 10-3 D)  4.00 × 10-4 E)  none of these" class="answers-bank-image d-inline" rel="preload" >
-What is the numerical value of the rate constant?

Accepted Answer

A)   4.00 × 10-1
B)   4.00 × 10-2
C)   4.00 × 10-3
D)   4.00 × 10-4
E)   none of theseF) None of the above
G) All of the above

Question 11

In the reaction
3A(g) + B(g) → 2C(g) + 4D(g)
the following data were collected at 100° C.  
Let Rate  
and use these data.
A. Determine the differential rate law. Be sure to label your plots carefully and show your work.
B. Calculate the value of the rate constant k for this reaction at 100°C.
C. Calculate [A] and [B] for experiment 1 after 5.00 × 102 s has elapsed.
D. Which of the following mechanisms could be correct for this reaction? Support your answer.

Accepted Answer

A. Rate = k[A][B]
B. 1.43 × 10^-3 L • mol^-1 •...

Question 12

The following initial rate data were found for the reaction
2MnO4- + 5H2C2O4 + 6H+ → 2Mn2+ + 10CO2 + 8H2O 4- + 5H2C2O4 + 6H+ → 2Mn2+ + 10CO2 + 8H2O   -For which order reaction is the half-life of the reaction independent of the initial concentration of the reactant(s) ? A)  zero order B)  first order C)  second order D)  all of these E)  none of these" class="answers-bank-image d-inline" rel="preload" >
-For which order reaction is the half-life of the reaction independent of the initial concentration of the reactant(s) ?

Accepted Answer

A)   zero order
B)   first order
C)   second order
D)   all of these
E)   none of theseF) A) and B)
G) A) and E)

Question 13

For the reaction in which A and B react to form C, the following initial rate data were obtained. 2[B]2 B)  Rate = k[A]2[B] C)  Rate = k[A][B]2 D)  Rate = k[A][B] E)  Rate = k[A]3" class="answers-bank-image d-inline" rel="preload" > What is the rate law for the reaction?

Accepted Answer

A)   Rate = k[A]2[B]2
B)   Rate = k[A]2[B]
C)   Rate = k[A][B]2
D)   Rate = k[A][B]
E)   Rate = k[A]3F) A) and D)
G) None of the above

Question 14

The reaction A → B + C is known to be zero order in A with a rate constant of 4.8 × 10-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]0 = 2.0M. What is the concentration of B after 4.0s?

Accepted Answer

A)   1.8M
B)   5.5× 10-1 M
C)   2.0M
D)   1.9× 10-1 M
E)   1.1× 10-1 MF) A) and B)
G) None of the above

Question 15

The following questions refer to the reaction 2A2 + B2 → 2C. The mechanism below has been proposed: 2 + B2 → 2C. The mechanism below has been proposed:   -Which step(s)  is(are)  rate-determining? A)  a step that is intermediate between step 1 and step 2 B)  both steps C)  step 2 D)  step 1 E)  none of these " class="answers-bank-image d-inline" rel="preload" >
-Which step(s)  is(are)  rate-determining?

Accepted Answer

A)   a step that is intermediate between step 1 and step 2
B)   both steps
C)   step 2
D)   step 1
E)   none of theseF) C) and D)
G) A) and D)

Question 16

For the reaction A + B → products, the following data were obtained. 2[B] B)  Rate = k[B] C)  Rate = k[A][B] D)  Rate = k[A] E)  Rate = k[A][B] 2" class="answers-bank-image d-inline" rel="preload" > What is the experimental rate law?

Accepted Answer

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

Question 17

The following questions refer to the reaction 2A2 + B2 → 2C. The mechanism below has been proposed: 2 + B2 → 2C. The mechanism below has been proposed:   -What is the molecularity of step 2? A)  The molecularity cannot be determined. B)  bimolecular C)  quadmolecular D)  unimolecular E)  termolecular" class="answers-bank-image d-inline" rel="preload" >
-What is the molecularity of step 2?

Accepted Answer

A)   The molecularity cannot be determined.
B)   bimolecular
C)   quadmolecular
D)   unimolecular
E)   termolecularF) None of the above
G) C) and D)

Question 18

At a particular temperature, N2O5 decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration of N2O5 is 1.0 × 1016 molecules/cm3, what will be the concentration in molecules/cm3 after 10.0 s?

Accepted Answer

A)   6.3 × 103
B)   9.9 × 1014
C)   9.4 × 102
D)   7.3 × 109
E)   1.8 × 1012F) All of the above
G) B) and E)

Question 19

The following questions refer to the hypothetical reaction A + B → products. The kinetics data given can be analyzed to answer the questions. -3 C)  4.3 × 10-3 D)  0.86 E)  1.2 × 10-2 " class="answers-bank-image d-inline" rel="preload" > ​
Determine the magnitude of the pseudo-rate constant (k')  if the magnitude of X in the rate data is 0.00905.

Accepted Answer

A)   0.31
B)   1.81 × 10-3
C)   4.3 × 10-3
D)   0.86
E)   1.2 × 10-2F) All of the above
G) A) and B)

Question 20

For the reaction
2A + B → products
the following mechanism is proposed:
A + B  M
A + M → products
Assuming that the second step is the rate-determining step and the first step is a fast equilibrium step, determine the rate law. Represent the rate constant in terms of k1, k-1, and k2.

Accepted Answer

Exam 15: Chemical Kinetics

The following initial rate data were found for the reaction 2MnO₄^- + 5H₂C₂O₄ + 6H⁺ → 2Mn²⁺ + 10CO₂ + 8H₂O -For which order reaction is the half-life of the reaction independent of the initial concentration of the reactant(s) ?

Correct Answer
verified

A general reaction written as 2A + 2B → C + 2D is studied and yields the following data. -What is the numerical value of the rate constant?

Correct Answer
verified

For the reaction CH₃CHCH₂(g) + HCl(g) → CH₃CHClCH₃(g) a possible mechanism is Fast equilibrium Fast equilibrium Complex + (HCl)₂ CH₃CHClCH₃ + 2HCl Slow Derive the rate law for this reaction using this mechanism.

Correct Answer
verified

Correct Answer
verified

The reaction A → B + C is known to be zero order in A with a rate constant of 4.8 × 10^-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]₀ = 2.0M. What is the concentration of B after 4.0s?

Correct Answer
verified

The following questions refer to the reaction 2A₂ + B₂ → 2C. The mechanism below has been proposed: -What is the molecularity of step 2?

Correct Answer
verified

The following questions refer to the hypothetical reaction A + B → products. The kinetics data given can be analyzed to answer the questions. Determine the magnitude of the pseudo-rate constant (k') if the magnitude of X in the rate data is 0.00905.

Correct Answer
verified

For the reaction A + B → products, the following data were obtained. What is the experimental rate law?

Correct Answer
verified

Correct Answer
verified
A. Rate = k[A][B]
B. 1.43 × 10^-3 L • mol^-1 •...
View Answer

At a particular temperature, N₂O₅ decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration of N₂O₅ is 1.0 × 10¹⁶ molecules/cm³, what will be the concentration in molecules/cm³ after 10.0 s?

Correct Answer
verified

For the reaction in which A and B react to form C, the following initial rate data were obtained. What is the rate law for the reaction?

Correct Answer
verified

For the reaction 2A + B → products the following mechanism is proposed: A + B M A + M → products Assuming that the second step is the rate-determining step and the first step is a fast equilibrium step, determine the rate law. Represent the rate constant in terms of k₁, k_-1, and k₂.

Correct Answer
verified

The following questions refer to the reaction 2A₂ + B₂ → 2C. The mechanism below has been proposed: -Which step(s) is(are) rate-determining?

Correct Answer
verified

Which quantity is greatest?

Correct Answer
verified

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

Correct Answer
verified

Use the potential energy diagram shown to answer the following questions. -Which letter shows the change in energy for the overall reaction?

Correct Answer
verified

Tabulated below are initial rate data for the reaction 2Fe(CN) ₆^3- + 2I^- → 2Fe(CN) ₆^4- + I₂ What is the experimental rate law?

Correct Answer
verified

The reaction 3NO → N₂O + NO₂ Is found to obey the rate law Rate = k[NO]². If the first half-life of the reaction is found to be 3.5 s, what is the length of the fourth half-life?

Correct Answer
verified

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

Correct Answer
verified

Consider the second-order reaction aA → products (which has a first half-life of 25 s) . If the concentration of A after 15.6s is 0.36M, determine the initial concentration of A.

Correct Answer
verified

Exam 15: Chemical Kinetics

The following initial rate data were found for the reaction 2MnO4- + 5H2C2O4 + 6H+ → 2Mn2+ + 10CO2 + 8H2O -For which order reaction is the half-life of the reaction independent of the initial concentration of the reactant(s) ?

Correct AnswerverifiedShow Answer

A general reaction written as 2A + 2B → C + 2D is studied and yields the following data. -What is the numerical value of the rate constant?

Correct AnswerverifiedShow Answer

For the reaction CH3CHCH2(g) + HCl(g) → CH3CHClCH3(g) a possible mechanism is Fast equilibrium Fast equilibrium Complex + (HCl)2 CH3CHClCH3 + 2HCl Slow Derive the rate law for this reaction using this mechanism.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The reaction A → B + C is known to be zero order in A with a rate constant of 4.8 × 10-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]0 = 2.0M. What is the concentration of B after 4.0s?

Correct AnswerverifiedShow Answer

The following questions refer to the reaction 2A2 + B2 → 2C. The mechanism below has been proposed: -What is the molecularity of step 2?

Correct AnswerverifiedShow Answer

The following questions refer to the hypothetical reaction A + B → products. The kinetics data given can be analyzed to answer the questions. ​ Determine the magnitude of the pseudo-rate constant (k') if the magnitude of X in the rate data is 0.00905.

Correct AnswerverifiedShow Answer

For the reaction A + B → products, the following data were obtained. What is the experimental rate law?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedA. Rate = k[A][B]B. 1.43 × 10-3 L • mol-1 •...View AnswerShow Answer

At a particular temperature, N2O5 decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration of N2O5 is 1.0 × 1016 molecules/cm3, what will be the concentration in molecules/cm3 after 10.0 s?

Correct AnswerverifiedShow Answer

For the reaction in which A and B react to form C, the following initial rate data were obtained. What is the rate law for the reaction?

Correct AnswerverifiedShow Answer

For the reaction 2A + B → products the following mechanism is proposed: A + B M A + M → products Assuming that the second step is the rate-determining step and the first step is a fast equilibrium step, determine the rate law. Represent the rate constant in terms of k1, k-1, and k2.

Correct AnswerverifiedShow Answer

The following questions refer to the reaction 2A2 + B2 → 2C. The mechanism below has been proposed: -Which step(s) is(are) rate-determining?

Correct AnswerverifiedShow Answer

Which quantity is greatest?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Use the potential energy diagram shown to answer the following questions. -Which letter shows the change in energy for the overall reaction?

Correct AnswerverifiedShow Answer

Tabulated below are initial rate data for the reaction 2Fe(CN) 63- + 2I- → 2Fe(CN) 64- + I2 What is the experimental rate law?

Correct AnswerverifiedShow Answer

The reaction 3NO → N2O + NO2 Is found to obey the rate law Rate = k[NO]2. If the first half-life of the reaction is found to be 3.5 s, what is the length of the fourth half-life?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Consider the second-order reaction aA → products (which has a first half-life of 25 s) . If the concentration of A after 15.6s is 0.36M, determine the initial concentration of A.

Correct AnswerverifiedShow Answer

The following initial rate data were found for the reaction 2MnO₄^- + 5H₂C₂O₄ + 6H⁺ → 2Mn²⁺ + 10CO₂ + 8H₂O -For which order reaction is the half-life of the reaction independent of the initial concentration of the reactant(s) ?

Correct Answer
verified

Correct Answer
verified

For the reaction CH₃CHCH₂(g) + HCl(g) → CH₃CHClCH₃(g) a possible mechanism is Fast equilibrium Fast equilibrium Complex + (HCl)₂ CH₃CHClCH₃ + 2HCl Slow Derive the rate law for this reaction using this mechanism.

Correct Answer
verified

Correct Answer
verified

The reaction A → B + C is known to be zero order in A with a rate constant of 4.8 × 10^-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]₀ = 2.0M. What is the concentration of B after 4.0s?

Correct Answer
verified

The following questions refer to the reaction 2A₂ + B₂ → 2C. The mechanism below has been proposed: -What is the molecularity of step 2?

Correct Answer
verified

The following questions refer to the hypothetical reaction A + B → products. The kinetics data given can be analyzed to answer the questions. Determine the magnitude of the pseudo-rate constant (k') if the magnitude of X in the rate data is 0.00905.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
A. Rate = k[A][B]
B. 1.43 × 10^-3 L • mol^-1 •...
View Answer

At a particular temperature, N₂O₅ decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration of N₂O₅ is 1.0 × 10¹⁶ molecules/cm³, what will be the concentration in molecules/cm³ after 10.0 s?

Correct Answer
verified

Correct Answer
verified

For the reaction 2A + B → products the following mechanism is proposed: A + B M A + M → products Assuming that the second step is the rate-determining step and the first step is a fast equilibrium step, determine the rate law. Represent the rate constant in terms of k₁, k_-1, and k₂.

Correct Answer
verified

The following questions refer to the reaction 2A₂ + B₂ → 2C. The mechanism below has been proposed: -Which step(s) is(are) rate-determining?

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

Tabulated below are initial rate data for the reaction 2Fe(CN) ₆^3- + 2I^- → 2Fe(CN) ₆^4- + I₂ What is the experimental rate law?

Correct Answer
verified

The reaction 3NO → N₂O + NO₂ Is found to obey the rate law Rate = k[NO]². If the first half-life of the reaction is found to be 3.5 s, what is the length of the fourth half-life?

Correct Answer
verified

Correct Answer
verified

Correct Answer
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