Question 1

For the reaction
P4(g) + 5O2(g) → 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[P...

Question 2

Rate constants are dependent upon

Accepted Answer

A)   the temperature
B)   the probability that a collision will have sufficient energy to cause a reaction
C)   the orientation of the collision
D)   the frequency of collisions
E)   all of the aboveF)  A and D onlyG) C) and E)
H) A) and B)

Question 3

The following data were obtained for the reaction of NO with O2. Concentrations are in molecules/cm3 and rates are in molecules/cm3 • s. 2. Concentrations are in molecules/cm3 and rates are in molecules/cm3 • s.   Which of the following is the correct rate law? A)  Rate = k[NO]2 B)  Rate = k[NO]2[O2]2 C)  Rate = k[NO][O2]2 D)  Rate = k[NO][O2] E)  Rate = k[NO]2[O2]" class="answers-bank-image d-inline" rel="preload" > Which of the following is the correct rate law?

Accepted Answer

A)   Rate = k[NO]2
B)   Rate = k[NO]2[O2]2
C)   Rate = k[NO][O2]2
D)   Rate = k[NO][O2]
E)   Rate = k[NO]2[O2]F) C) and D)
G) None of the above

Question 4

Consider the reaction
3A + B + C → D + E
Where the rate law is defined as 0 = [C]0 = 1.00 M and [A]0 = 2.46× 10-4 M. After 2.96 min, [A] = 3.20× 10-5 M. What is the value of k? A)  8.30× 107 L3/mol3 • s B)  4.02× 10-7 L3/mol3 • s C)  2.14× 10-5 L3/mol3 • s D)  1.53× 102 L3/mol3 • s E)  9.18× 103 L3/mol3 • s" class="answers-bank-image d-inline" rel="preload" >
An experiment is carried out where [B]0 = [C]0 = 1.00 M and [A]0 = 2.46× 10-4 M. After 2.96 min, [A] = 3.20× 10-5 M. What is the value of k?

Accepted Answer

A)   8.30× 107 L3/mol3 • s
B)   4.02× 10-7 L3/mol3 • s
C)   2.14× 10-5 L3/mol3 • s
D)   1.53× 102 L3/mol3 • s
E)   9.18× 103 L3/mol3 • sF) A) and D)
G) C) and D)

Question 5

The reaction
2N2O5(g)  → O2(g)  + 4NO2(g) 
Is first order in N2O5. For this reaction at 45° C, the rate constant k = 1.0 × 10-5 s-1, where the rate law is defined as
Rate 2O5(g)  → O2(g)  + 4NO2(g)  Is first order in N2O5. For this reaction at 45° C, the rate constant k = 1.0 × 10-5 s-1, where the rate law is defined as Rate   For a particular experiment ([N2O5]0 = 1.0 × 10-3 M) , calculate [N2O5] after 1.0 × 105 s. A)  0 B)  5.0 × 10-4 M C)  3.7 × 10-4 M D)  1.0 × 10-3 M E)  none of these" class="answers-bank-image d-inline" rel="preload" >
For a particular experiment ([N2O5]0 = 1.0 × 10-3 M) , calculate [N2O5] after 1.0 × 105 s.

Accepted Answer

A)   0
B)   5.0 × 10-4 M
C)   3.7 × 10-4 M
D)   1.0 × 10-3 M
E)   none of theseF) A) and B)
G) A) and D)

Question 6

For the reaction aA → products, select the reaction order(s)  that best fit(s)  the observations.
-The half-life decreases over time.

Accepted Answer

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

Question 7

For the reaction
2A + B → products
the following mechanism is proposed:
A + B  M
A + M → products
Using the steady-state approximation, determine the rate law.

Accepted Answer

rate = k₁k₂ ...

Question 8

The reaction
2A + B → 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 → E
Step 3: E + A → 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]2F) A) and E)
G) None of the above

Question 9

The following data were collected in two studies of the reaction below.A + 2B → C + D  ​
Which of the following mechanisms could be correct for this reaction?

Accepted Answer

A)   A + A → E (slow) E + B → C + D (fast) 
B)   A + B  E (fast) E + B → C + D (slow) 
C)   A + B  E (fast) E + A → C + D (slow) 
D)   none of theseE) All of the above
F) B) and C)

Question 10

The following questions refer to the hypothetical reaction A + B → products. The kinetics data given can be analyzed to answer the questions. x B)  Rate = k'[A]x[B]y C)  Rate = kk'[B]y D)  Rate = k'[B]y E)  Rate = k'[A]x" class="answers-bank-image d-inline" rel="preload" >
-What form will the pseudo-rate law have?

Accepted Answer

A)   Rate = kk'[A]x
B)   Rate = k'[A]x[B]y
C)   Rate = kk'[B]y
D)   Rate = k'[B]y
E)   Rate = k'[A]xF) B) and D)
G) A) and E)

Question 11

The oxidation of Cr3+ to CrO42- can be accomplished using Ce4+ in a buffered solution. The following data were obtained: 3+ to CrO42- can be accomplished using Ce4+ in a buffered solution. The following data were obtained:   -Determine the order in the rate law of the species Cr3+. A)  -2 B)  3 C)  1 D)  2 E)  -1" class="answers-bank-image d-inline" rel="preload" >
-Determine the order in the rate law of the species Cr3+.

Accepted Answer

A)   -2
B)   3
C)   1
D)   2
E)   -1F) C) and D)
G) B) and E)

Question 12

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

Accepted Answer

The answer of A reaction represented by the equation
3OS1U1B12S1U1B0(g) →...

Question 13

In 6 M HCl, the complex ion Ru(NH3) 63+ decomposes to a variety of products. The reaction is first order in Ru(NH3) 63+ and has a half-life of 14 h at 25°C. Under these conditions, how long will it take for the [Ru(NH3) 63+] to decrease to 39.0% of its initial value?

Accepted Answer

A)   4.3h
B)   10h
C)   8.3h
D)   19h
E)   5.5hF) C) and D)
G) B) and D)

Question 14

Which of the following statement is/are true of rate law?
1)  The proportionality constant k, called the rate constant, and n, called the order of the reactant in the rate law, must be determined by experiment.
2)  The concentrations of the products of a chemical reaction do not appear in the rate law.
3)  The order of a reactant in the rate law can only be a positive integer.

Accepted Answer

A)   1 only​
B)   2 only​
C)   3 only​
D)   1 and 2​
E)   2 and 3​F) C) and D)
G) A) and B)

Question 15

For the reaction aA → products, select the reaction order(s)  that best fit(s)  the observations.
-The reaction A → B + C is known to be zero order in A with a rate constant of 5.2 × 10-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]0 = 3.2 × 10-3 M. What is the half-life for the reaction?

Accepted Answer

A)   1.3× 101 s
B)   2.6× 10-2 s
C)   8.3× 10-2 s
D)   6.0× 104 s
E)   3.1× 10-2 sF) C) and E)
G) None of the above

Question 16

For which of the following is the half-life directly dependent on the concentration of the reactant?

Accepted Answer

A)   zero-order reaction
B)   second-order reaction
C)   first-order reaction
D)   two of these
E)   all of theseF) A) and C)
G) A) and E)

Question 17

At a particular temperature, the half-life of a zero-order reaction is 29.0min. How long will it take for the reactant concentration to be depleted by a factor of 8?

Accepted Answer

A)   87.0min
B)   58.0min
C)   50.8min
D)   232min
E)   203minF) C) and D)
G) A) and C)

Question 18

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

Accepted Answer

A) True 
 B)False

Question 19

If the reaction 2HI → H2 + I2 is second order, which of the following will yield a linear plot?

Accepted Answer

A)   log [HI] vs. time
B)   [HI] vs. time
C)   ln [HI] vs. time
D)   1/[HI] vs. timeE) All of the above
F) A) and B)

Question 20

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 initial rate of production of NO2 for this reaction is approximately A)  6.4 × 10-4 mol/L • min B)  3.2 × 10-4 mol/L • min C)  1.24 × 10-2 mol/L • min D)  1.6 × 10-4 mol/L • min E)  none of these" class="answers-bank-image d-inline" rel="preload" > The initial rate of production of NO2 for this reaction is approximately

Accepted Answer

A)   6.4 × 10-4 mol/L • min
B)   3.2 × 10-4 mol/L • min
C)   1.24 × 10-2 mol/L • min
D)   1.6 × 10-4 mol/L • min
E)   none of theseF) All of the above
G) D) and E)

Exam 15: Chemical Kinetics

In 6 M HCl, the complex ion Ru(NH₃) ₆³⁺ decomposes to a variety of products. The reaction is first order in Ru(NH₃) ₆³⁺ and has a half-life of 14 h at 25°C. Under these conditions, how long will it take for the [Ru(NH₃) ₆³⁺] to decrease to 39.0% of its initial value?

Correct Answer
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The following questions refer to the hypothetical reaction A + B → products. The kinetics data given can be analyzed to answer the questions. -What form will the pseudo-rate law have?

Correct Answer
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The following data were obtained for the reaction of NO with O₂. Concentrations are in molecules/cm³ and rates are in molecules/cm³ • s. Which of the following is the correct rate law?

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

Correct Answer
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Correct Answer
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The following data were collected in two studies of the reaction below.A + 2B → C + D Which of the following mechanisms could be correct for this reaction?

Correct Answer
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For the reaction P₄(g) + 5O₂(g) → 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 Answer
verified
Rate = k[P...
View Answer

At a particular temperature, the half-life of a zero-order reaction is 29.0min. How long will it take for the reactant concentration to be depleted by a factor of 8?

Correct Answer
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For the reaction 2N₂O₅(g) → 4NO₂(g) + O₂(g) , the following data were collected. The initial rate of production of NO₂ for this reaction is approximately

Correct Answer
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For which of the following is the half-life directly dependent on the concentration of the reactant?

Correct Answer
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For the reaction aA → products, select the reaction order(s) that best fit(s) the observations. -The half-life decreases over time.

Correct Answer
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For the reaction 2A + B → products the following mechanism is proposed: A + B M A + M → products Using the steady-state approximation, determine the rate law.

Correct Answer
verified
rate = k₁k₂ ...
View Answer

Consider the reaction 3A + B + C → D + E Where the rate law is defined as An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 2.46× 10^-4 M. After 2.96 min, [A] = 3.20× 10^-5 M. What is the value of k?

Correct Answer
verified

The reaction 2N₂O₅(g) → O₂(g) + 4NO₂(g) Is first order in N₂O₅. For this reaction at 45° C, the rate constant k = 1.0 × 10^-5 s^-1, where the rate law is defined as Rate For a particular experiment ([N₂O₅]₀ = 1.0 × 10^-3 M) , calculate [N₂O₅] after 1.0 × 10⁵ s.

Correct Answer
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If the reaction 2HI → H₂ + I₂ is second order, which of the following will yield a linear plot?

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

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

Correct Answer
verified

Rate constants are dependent upon

Correct Answer
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The oxidation of Cr³⁺ to CrO₄^2- can be accomplished using Ce⁴⁺ in a buffered solution. The following data were obtained: -Determine the order in the rate law of the species Cr³⁺.

Correct Answer
verified

Exam 15: Chemical Kinetics

In 6 M HCl, the complex ion Ru(NH3) 63+ decomposes to a variety of products. The reaction is first order in Ru(NH3) 63+ and has a half-life of 14 h at 25°C. Under these conditions, how long will it take for the [Ru(NH3) 63+] to decrease to 39.0% of its initial value?

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. -What form will the pseudo-rate law have?

Correct AnswerverifiedShow Answer

The following data were obtained for the reaction of NO with O2. Concentrations are in molecules/cm3 and rates are in molecules/cm3 • s. Which of the following is the correct rate law?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The following data were collected in two studies of the reaction below.A + 2B → C + D ​ Which of the following mechanisms could be correct for this reaction?

Correct AnswerverifiedShow Answer

For the reaction P4(g) + 5O2(g) → 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[P...View AnswerShow Answer

At a particular temperature, the half-life of a zero-order reaction is 29.0min. How long will it take for the reactant concentration to be depleted by a factor of 8?

Correct AnswerverifiedShow Answer

For the reaction 2N2O5(g) → 4NO2(g) + O2(g) , the following data were collected. The initial rate of production of NO2 for this reaction is approximately

Correct AnswerverifiedShow Answer

For which of the following is the half-life directly dependent on the concentration of the reactant?

Correct AnswerverifiedShow Answer

For the reaction aA → products, select the reaction order(s) that best fit(s) the observations. -The half-life decreases over time.

Correct AnswerverifiedShow Answer

For the reaction 2A + B → products the following mechanism is proposed: A + B M A + M → products Using the steady-state approximation, determine the rate law.

Correct Answerverifiedrate = k1k2 ...View AnswerShow Answer

Consider the reaction 3A + B + C → D + E Where the rate law is defined as An experiment is carried out where [B]0 = [C]0 = 1.00 M and [A]0 = 2.46× 10-4 M. After 2.96 min, [A] = 3.20× 10-5 M. What is the value of k?

Correct AnswerverifiedShow Answer

The reaction 2N2O5(g) → O2(g) + 4NO2(g) Is first order in N2O5. For this reaction at 45° C, the rate constant k = 1.0 × 10-5 s-1, where the rate law is defined as Rate For a particular experiment ([N2O5]0 = 1.0 × 10-3 M) , calculate [N2O5] after 1.0 × 105 s.

Correct AnswerverifiedShow Answer

If the reaction 2HI → H2 + I2 is second order, which of the following will yield a linear plot?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Rate constants are dependent upon

Correct AnswerverifiedShow Answer

The oxidation of Cr3+ to CrO42- can be accomplished using Ce4+ in a buffered solution. The following data were obtained: -Determine the order in the rate law of the species Cr3+.

Correct AnswerverifiedShow Answer

In 6 M HCl, the complex ion Ru(NH₃) ₆³⁺ decomposes to a variety of products. The reaction is first order in Ru(NH₃) ₆³⁺ and has a half-life of 14 h at 25°C. Under these conditions, how long will it take for the [Ru(NH₃) ₆³⁺] to decrease to 39.0% of its initial value?

Correct Answer
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Correct Answer
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The following data were obtained for the reaction of NO with O₂. Concentrations are in molecules/cm³ and rates are in molecules/cm³ • s. Which of the following is the correct rate law?

Correct Answer
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Correct Answer
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Correct Answer
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The following data were collected in two studies of the reaction below.A + 2B → C + D Which of the following mechanisms could be correct for this reaction?

Correct Answer
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For the reaction P₄(g) + 5O₂(g) → 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 Answer
verified
Rate = k[P...
View Answer

Correct Answer
verified

For the reaction 2N₂O₅(g) → 4NO₂(g) + O₂(g) , the following data were collected. The initial rate of production of NO₂ for this reaction is approximately

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 = k₁k₂ ...
View Answer

Consider the reaction 3A + B + C → D + E Where the rate law is defined as An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 2.46× 10^-4 M. After 2.96 min, [A] = 3.20× 10^-5 M. What is the value of k?

Correct Answer
verified

The reaction 2N₂O₅(g) → O₂(g) + 4NO₂(g) Is first order in N₂O₅. For this reaction at 45° C, the rate constant k = 1.0 × 10^-5 s^-1, where the rate law is defined as Rate For a particular experiment ([N₂O₅]₀ = 1.0 × 10^-3 M) , calculate [N₂O₅] after 1.0 × 10⁵ s.

Correct Answer
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If the reaction 2HI → H₂ + I₂ is second order, which of the following will yield a linear plot?

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

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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The oxidation of Cr³⁺ to CrO₄^2- can be accomplished using Ce⁴⁺ in a buffered solution. The following data were obtained: -Determine the order in the rate law of the species Cr³⁺.

Correct Answer
verified