Question 1

-What is the activation energy for the formation of ozone?

Accepted Answer

A)  14 kJ
B)  392 kJ
C)  406 kJ
D)  none of theseE) A) and D)
F) None of the above

Question 2

A gaseous reaction occurs by a two-step mechanism,shown below.
Step 1: AX +Y2 ⇌ AXY2 fast
Step 2: AXY2 + AX → 2 AXY slow
Including concentration of only reactants and products,what is the rate law for this reaction?

Accepted Answer

A)  Rate = k[AX][Y2]
B)  Rate = k[AXY2]/[AX][Y2]
C)  Rate = k[AX]2[Y2]
D)  Rate = k[AXY]2/[AXY2][AX]E) A) and C)
F) A) and B)

Question 3

A plot of 1/[BrO-] vs time is linear for the reaction:
3 BrO-(aq) → BrO3-(aq) + 2 Br-(aq) 
What is the order of the reaction with respect to the hypobromite ion,BrO-?

Accepted Answer

A)  0
B)  1
C)  2
D)  3E) A) and B)
F) C) and D)

Question 4

Cerium(IV) ion reacts with thallium(I) ion in a one-step reaction shown below:
2 Ce4+(aq) + Tl+(aq) → 2 Ce3+(aq) + Tl3+(aq) .
If the rate law is: Rate = k[Ce4+]2[Tl+],what is the overall order of the reaction?

Accepted Answer

A)  first
B)  second
C)  third
D)  fourthE) All of the above
F) A) and C)

Question 5

For the zeroth-order reaction: C → products,-Δ[C]/Δt = k,which of the following graphs would be expected to give a straight line?

Accepted Answer

A)  [C] vs.t
B)  ln[C] vs.t
C)  1/[C] vs.t
D)  [C]2 vs.tE) B) and C)
F) A) and B)

Question 6

Hydrogen iodide decomposes at 800 K via a second-order process to produce hydrogen and iodine according to the following chemical equation.
2 HI(g) → H2(g) + I2(g) 
At 800 K it takes 142 seconds for the initial concentration of HI to decrease from 6.75 × 10-2 M to 3.50 × 10-2 M.What is the rate constant for the reaction at this temperature?

Accepted Answer

A)  5) 12 × 10-4 M-1s-1
B)  9) 69 × 10-2 M-1s-1
C)  10.3 M-1s-1
D)  1) 95 × 103 M-1s-1E) C) and D)
F) A) and D)

Question 7

Which statement below regarding the half-life of a second-order reaction is true?

Accepted Answer

A)  Each half-life is half as long as the preceding one.
B)  Each half-life is twice as long as the preceding one.
C)  Each half-life is four times as long as the preceding one.
D)  The length of the half-life remains unchanged throughout the course of the reaction.E) B) and C)
F) A) and D)

Question 8

The following set of data was obtained by the method of initial rates for the reaction:
(H3C) 3CBr + OH- → (H3C) 3COH + Br-
What is the value of the rate constant,k? 3C) 3CBr + OH- → (H3C) 3COH + Br- What is the value of the rate constant,k?   A) 8) 8 × 10-4 s-1 B) 4) 4 × 10-4 s-1 C) 1) 8 × 10-4 s-1 D) none of these" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  8) 8 × 10-4 s-1
B)  4) 4 × 10-4 s-1
C)  1) 8 × 10-4 s-1
D)  none of theseE) A) and D)
F) A) and C)

Question 9

The first-order isomerization reaction: cyclopropane → propene,has a rate constant of
1) 10 × 10-4s-1 at 470°C and an activation energy of 264 kJ/mol.What is the temperature of the reaction when the rate constant is equal to 4.36 × 10-3s-1?

Accepted Answer

A)  126°C
B)  411°C
C)  510°C
D)  540°CE) None of the above
F) B) and D)

Question 10

A reaction has the rate law Rate = k[NO]2[H2].If the concentration of NO is reduced by half and the concentration of H2 is quadrupled,the rate of reaction will ________ (increase,decrease,not change).

Accepted Answer

Question 11

The reaction for the decomposition of dinitrogen monoxide gas to form oxygen radicals is:
N2O(g)   →\rarr→  N2(g) + O(g) .If the rate constant is 3.04 × 10-2 s-1 and the frequency factor is
8) 00 × 1011 s-1,what is the activation energy for the first-order reaction at 700°C?

Accepted Answer

A)  0) 262 kJ/mol
B)  38.2 kJ/mol
C)  180 kJ/mol
D)  250 kJ/mol E) None of the above
F) A) and C)

Question 12

Consider the first-order reaction A → B in which A molecules (shaded spheres) are converted to B molecules (unshaded spheres) . 
-Which drawing (a) -(d) represents the reaction mixture at t = 3 minutes?

Accepted Answer

A)  drawing (a) 
B)  drawing (b) 
C)  drawing (c) 
D)  drawing (d) E) A) and B)
F) A) and C)

Question 13

For the reaction shown below,what is the relationship between the rate of formation of Br2 and the rate of reaction of Br- over the same time period?
ClO2-(aq) + 4 Br-(aq) + 4 H+(aq) → Cl-(aq) + 2 Br2(aq) +2 H2O(l)

Accepted Answer

A)  rate of formation of Br2 = 1/2 × rate of reaction of Br-
B)  rate of formation of Br2 = 1/4 × rate of reaction of Br-
C)  rate of formation of Br2 = 2 × rate of reaction of Br-
D)  Rate of formation of Br2 = 2 × rate of reaction of Br-E) A) and B)
F) None of the above

Question 14

The decomposition of ozone in the stratosphere can occur by the following two-step mechanism:
Br + O3 → BrO + O2
BrO + O → Br + O2
Which species is a catalyst in this mechanism?

Accepted Answer

A)  Br
B)  BrO
C)  O
D)  O3E) B) and C)
F) C) and D)

Question 15

A mechanism for a naturally occurring reaction that destroys ozone is:
Step 1: O3(g) + HO(g) → HO2(g) + O2(g) 
Step 2: HO2(g) + O(g) → HO(g) + O2(g) 
What is the molecularity of the overall reaction?

Accepted Answer

A)  unimolecular
B)  bimolecular
C)  none of these because molecularity is the difference of the exponents in the rate law
D)  none of these because molecularity only refers to elementary stepsE) None of the above
F) A) and B)

Question 16

The reaction below is first order in H2 and one-half order in Br2.The rate law for this reaction is ________.
H2(g)+ Br2(g)→ 2 HBr(g)

Accepted Answer

Question 17

For the first-order reaction,2 N2O(g) → 2 N2(g) + O2(g) ,what is the concentration of N2O after 3 half-lives if 0.25 mol of N2O is initially placed into a 1.00-L reaction vessel?

Accepted Answer

A)  1) 6 × 10- 2 M
B)  3) 1 × 10- 2 M
C)  6) 2 × 10- 2 M
D)  1) 2 × 10- 1 ME) All of the above
F) A) and D)

Question 18

A concentration-time study of the gas phase reaction 2 A3 → 3 A2 produced the data in the table below.
Time (s) [A3] (M) [A2] (M) 
0 4) 00 × 10-4 0
10 2.00 × 10-4 3.00 × 10-4
20 1.00 × 10-4 4.50 × 10-4
30 5.00 × 10-5 ?
What is the concentration of A2 after 30 seconds?

Accepted Answer

A)  5) 00 × 10-4 M
B)  5) 25 × 10-4 M
C)  5) 50 × 10-4 M
D)  6) 00 × 10-4 ME) All of the above
F) B) and D)

Question 19

Methanol can be produced by the following reaction:
CO(g) + 2 H2(g) → CH3OH(g) .
How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol? 2(g) → CH3OH(g) . How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol?   = ? A)    B)    C)    D) none of these" class="answers-bank-image d-inline" rel="preload" >
= ?

Accepted Answer

A)   2(g) → CH3OH(g) . How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol?   = ? 
A)     
B)     
C)     
D)  none of these" class="answers-bank-image d-inline" rel="preload" >
B)   2(g) → CH3OH(g) . How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol?   = ? 
A)     
B)     
C)     
D)  none of these" class="answers-bank-image d-inline" rel="preload" >
C)   2(g) → CH3OH(g) . How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol?   = ? 
A)     
B)     
C)     
D)  none of these" class="answers-bank-image d-inline" rel="preload" >
D)  none of theseE) B) and D)
F) A) and C)

Question 20

Hydrogen peroxide decomposes to water and oxygen according to the reaction below:
2 H2O2(aq) → 2 H2O(l) + O2(g) 
In the presence of large excesses of I- ion,the following set of data is obtained.What is the average rate of disappearance of H2O2(aq) in M/s in the first 45.0 seconds of the reaction if 1.00 L of H2O2 reacts at 25°C and 1.00 atm pressure? 2O2(aq) → 2 H2O(l) + O2(g)  In the presence of large excesses of I- ion,the following set of data is obtained.What is the average rate of disappearance of H2O2(aq) in M/s in the first 45.0 seconds of the reaction if 1.00 L of H2O2 reacts at 25°C and 1.00 atm pressure?   A) 9) 09 × 10-7 M/s B) 3) 63 × 10-6 M/s C) 4) 33 × 10-5 M/s D) 1) 64 × 10-4 M/s" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  9) 09 × 10-7 M/s
B)  3) 63 × 10-6 M/s
C)  4) 33 × 10-5 M/s
D)  1) 64 × 10-4 M/sE) B) and C)
F) A) and C)

Exam 12: Chemical Kinetics

Consider the first-order reaction A → B in which A molecules (shaded spheres) are converted to B molecules (unshaded spheres) . -Which drawing (a) -(d) represents the reaction mixture at t = 3 minutes?

Correct Answer
verified

For the reaction shown below,what is the relationship between the rate of formation of Br₂ and the rate of reaction of Br^- over the same time period? ClO₂^-(aq) + 4 Br^-(aq) + 4 H⁺(aq) → Cl^-(aq) + 2 Br₂(aq) +2 H₂O(l)

Correct Answer
verified

Which statement below regarding the half-life of a second-order reaction is true?

Correct Answer
verified

The decomposition of ozone in the stratosphere can occur by the following two-step mechanism: Br + O₃ → BrO + O₂ BrO + O → Br + O₂ Which species is a catalyst in this mechanism?

Correct Answer
verified

Correct Answer
verified

For the first-order reaction,2 N₂O(g) → 2 N₂(g) + O₂(g) ,what is the concentration of N₂O after 3 half-lives if 0.25 mol of N₂O is initially placed into a 1.00-L reaction vessel?

Correct Answer
verified

-What is the activation energy for the formation of ozone?

Correct Answer
verified

The reaction for the decomposition of dinitrogen monoxide gas to form oxygen radicals is: N₂O(g) $\rarr$ N₂(g) + O(g) .If the rate constant is 3.04 × 10^-2 s^-1 and the frequency factor is 8) 00 × 10¹¹ s^-1,what is the activation energy for the first-order reaction at 700°C?

Correct Answer
verified

The following set of data was obtained by the method of initial rates for the reaction: (H₃C) ₃CBr + OH^- → (H₃C) ₃COH + Br^- What is the value of the rate constant,k?

Correct Answer
verified

A mechanism for a naturally occurring reaction that destroys ozone is: Step 1: O₃(g) + HO(g) → HO₂(g) + O₂(g) Step 2: HO₂(g) + O(g) → HO(g) + O₂(g) What is the molecularity of the overall reaction?

Correct Answer
verified

The reaction below is first order in H₂ and one-half order in Br₂.The rate law for this reaction is ________. H₂(g)+ Br₂(g)→ 2 HBr(g)

Correct Answer
verified

A gaseous reaction occurs by a two-step mechanism,shown below. Step 1: AX +Y₂ ⇌ AXY_{2 fast} Step 2: AXY₂ + AX → 2 AXY slow Including concentration of only reactants and products,what is the rate law for this reaction?

Correct Answer
verified

Methanol can be produced by the following reaction: CO(g) + 2 H₂(g) → CH₃OH(g) . How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol? = ?

Correct Answer
verified

The first-order isomerization reaction: cyclopropane → propene,has a rate constant of 1) 10 × 10^-4s^-1 at 470°C and an activation energy of 264 kJ/mol.What is the temperature of the reaction when the rate constant is equal to 4.36 × 10^-³s^-1?

Correct Answer
verified

A concentration-time study of the gas phase reaction 2 A₃ → 3 A₂ produced the data in the table below. Time (s) [A₃] (M) [A₂] (M) 0 4) 00 × 10^-4 0 10 2.00 × 10^-4 3.00 × 10^-4 20 1.00 × 10^-4 4.50 × 10^-4 30 5.00 × 10^-5 ? What is the concentration of A₂ after 30 seconds?

Correct Answer
verified

For the zeroth-order reaction: C → products,-Δ[C]/Δt = k,which of the following graphs would be expected to give a straight line?

Correct Answer
verified

A plot of 1/[BrO^-] vs time is linear for the reaction: 3 BrO^-(aq) → BrO₃^-(aq) + 2 Br^-(aq) What is the order of the reaction with respect to the hypobromite ion,BrO^-?

Correct Answer
verified

A reaction has the rate law Rate = k[NO]²[H₂].If the concentration of NO is reduced by half and the concentration of H₂ is quadrupled,the rate of reaction will ________ (increase,decrease,not change).

Correct Answer
verified

Cerium(IV) ion reacts with thallium(I) ion in a one-step reaction shown below: 2 Ce⁴⁺(aq) + Tl⁺(aq) → 2 Ce³⁺(aq) + Tl³⁺(aq) . If the rate law is: Rate = k[Ce⁴⁺]²[Tl⁺],what is the overall order of the reaction?

Correct Answer
verified

Correct Answer
verified

Exam 12: Chemical Kinetics

Consider the first-order reaction A → B in which A molecules (shaded spheres) are converted to B molecules (unshaded spheres) . -Which drawing (a) -(d) represents the reaction mixture at t = 3 minutes?

Correct AnswerverifiedShow Answer

For the reaction shown below,what is the relationship between the rate of formation of Br2 and the rate of reaction of Br- over the same time period? ClO2-(aq) + 4 Br-(aq) + 4 H+(aq) → Cl-(aq) + 2 Br2(aq) +2 H2O(l)

Correct AnswerverifiedShow Answer

Which statement below regarding the half-life of a second-order reaction is true?

Correct AnswerverifiedShow Answer

The decomposition of ozone in the stratosphere can occur by the following two-step mechanism: Br + O3 → BrO + O2 BrO + O → Br + O2 Which species is a catalyst in this mechanism?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

For the first-order reaction,2 N2O(g) → 2 N2(g) + O2(g) ,what is the concentration of N2O after 3 half-lives if 0.25 mol of N2O is initially placed into a 1.00-L reaction vessel?

Correct AnswerverifiedShow Answer

-What is the activation energy for the formation of ozone?

Correct AnswerverifiedShow Answer

The reaction for the decomposition of dinitrogen monoxide gas to form oxygen radicals is: N2O(g) →\rarr→ N2(g) + O(g) .If the rate constant is 3.04 × 10-2 s-1 and the frequency factor is 8) 00 × 1011 s-1,what is the activation energy for the first-order reaction at 700°C?

Correct AnswerverifiedShow Answer

The following set of data was obtained by the method of initial rates for the reaction: (H3C) 3CBr + OH- → (H3C) 3COH + Br- What is the value of the rate constant,k?

Correct AnswerverifiedShow Answer

A mechanism for a naturally occurring reaction that destroys ozone is: Step 1: O3(g) + HO(g) → HO2(g) + O2(g) Step 2: HO2(g) + O(g) → HO(g) + O2(g) What is the molecularity of the overall reaction?

Correct AnswerverifiedShow Answer

The reaction below is first order in H2 and one-half order in Br2.The rate law for this reaction is ________. H2(g)+ Br2(g)→ 2 HBr(g)

Correct AnswerverifiedShow Answer

A gaseous reaction occurs by a two-step mechanism,shown below. Step 1: AX +Y2 ⇌ AXY2 fast Step 2: AXY2 + AX → 2 AXY slow Including concentration of only reactants and products,what is the rate law for this reaction?

Correct AnswerverifiedShow Answer

Methanol can be produced by the following reaction: CO(g) + 2 H2(g) → CH3OH(g) . How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol? = ?

Correct AnswerverifiedShow Answer

The first-order isomerization reaction: cyclopropane → propene,has a rate constant of 1) 10 × 10-4s-1 at 470°C and an activation energy of 264 kJ/mol.What is the temperature of the reaction when the rate constant is equal to 4.36 × 10-3s-1?

Correct AnswerverifiedShow Answer

A concentration-time study of the gas phase reaction 2 A3 → 3 A2 produced the data in the table below. Time (s) [A3] (M) [A2] (M) 0 4) 00 × 10-4 0 10 2.00 × 10-4 3.00 × 10-4 20 1.00 × 10-4 4.50 × 10-4 30 5.00 × 10-5 ? What is the concentration of A2 after 30 seconds?

Correct AnswerverifiedShow Answer

For the zeroth-order reaction: C → products,-Δ[C]/Δt = k,which of the following graphs would be expected to give a straight line?

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A plot of 1/[BrO-] vs time is linear for the reaction: 3 BrO-(aq) → BrO3-(aq) + 2 Br-(aq) What is the order of the reaction with respect to the hypobromite ion,BrO-?

Correct AnswerverifiedShow Answer

A reaction has the rate law Rate = k[NO]2[H2].If the concentration of NO is reduced by half and the concentration of H2 is quadrupled,the rate of reaction will ________ (increase,decrease,not change).

Correct AnswerverifiedShow Answer

Cerium(IV) ion reacts with thallium(I) ion in a one-step reaction shown below: 2 Ce4+(aq) + Tl+(aq) → 2 Ce3+(aq) + Tl3+(aq) . If the rate law is: Rate = k[Ce4+]2[Tl+],what is the overall order of the reaction?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Correct Answer
verified

For the reaction shown below,what is the relationship between the rate of formation of Br₂ and the rate of reaction of Br^- over the same time period? ClO₂^-(aq) + 4 Br^-(aq) + 4 H⁺(aq) → Cl^-(aq) + 2 Br₂(aq) +2 H₂O(l)

Correct Answer
verified

Correct Answer
verified

The decomposition of ozone in the stratosphere can occur by the following two-step mechanism: Br + O₃ → BrO + O₂ BrO + O → Br + O₂ Which species is a catalyst in this mechanism?

Correct Answer
verified

Correct Answer
verified

For the first-order reaction,2 N₂O(g) → 2 N₂(g) + O₂(g) ,what is the concentration of N₂O after 3 half-lives if 0.25 mol of N₂O is initially placed into a 1.00-L reaction vessel?

Correct Answer
verified

Correct Answer
verified

The reaction for the decomposition of dinitrogen monoxide gas to form oxygen radicals is: N₂O(g) $\rarr$ N₂(g) + O(g) .If the rate constant is 3.04 × 10^-2 s^-1 and the frequency factor is 8) 00 × 10¹¹ s^-1,what is the activation energy for the first-order reaction at 700°C?

Correct Answer
verified

The following set of data was obtained by the method of initial rates for the reaction: (H₃C) ₃CBr + OH^- → (H₃C) ₃COH + Br^- What is the value of the rate constant,k?

Correct Answer
verified

A mechanism for a naturally occurring reaction that destroys ozone is: Step 1: O₃(g) + HO(g) → HO₂(g) + O₂(g) Step 2: HO₂(g) + O(g) → HO(g) + O₂(g) What is the molecularity of the overall reaction?

Correct Answer
verified

The reaction below is first order in H₂ and one-half order in Br₂.The rate law for this reaction is ________. H₂(g)+ Br₂(g)→ 2 HBr(g)

Correct Answer
verified

A gaseous reaction occurs by a two-step mechanism,shown below. Step 1: AX +Y₂ ⇌ AXY_{2 fast} Step 2: AXY₂ + AX → 2 AXY slow Including concentration of only reactants and products,what is the rate law for this reaction?

Correct Answer
verified

Methanol can be produced by the following reaction: CO(g) + 2 H₂(g) → CH₃OH(g) . How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol? = ?

Correct Answer
verified

The first-order isomerization reaction: cyclopropane → propene,has a rate constant of 1) 10 × 10^-4s^-1 at 470°C and an activation energy of 264 kJ/mol.What is the temperature of the reaction when the rate constant is equal to 4.36 × 10^-³s^-1?

Correct Answer
verified

A concentration-time study of the gas phase reaction 2 A₃ → 3 A₂ produced the data in the table below. Time (s) [A₃] (M) [A₂] (M) 0 4) 00 × 10^-4 0 10 2.00 × 10^-4 3.00 × 10^-4 20 1.00 × 10^-4 4.50 × 10^-4 30 5.00 × 10^-5 ? What is the concentration of A₂ after 30 seconds?

Correct Answer
verified

Correct Answer
verified

A plot of 1/[BrO^-] vs time is linear for the reaction: 3 BrO^-(aq) → BrO₃^-(aq) + 2 Br^-(aq) What is the order of the reaction with respect to the hypobromite ion,BrO^-?

Correct Answer
verified

A reaction has the rate law Rate = k[NO]²[H₂].If the concentration of NO is reduced by half and the concentration of H₂ is quadrupled,the rate of reaction will ________ (increase,decrease,not change).

Correct Answer
verified

Cerium(IV) ion reacts with thallium(I) ion in a one-step reaction shown below: 2 Ce⁴⁺(aq) + Tl⁺(aq) → 2 Ce³⁺(aq) + Tl³⁺(aq) . If the rate law is: Rate = k[Ce⁴⁺]²[Tl⁺],what is the overall order of the reaction?

Correct Answer
verified

Correct Answer
verified