Question 1

The rate constant of a first-order decomposition reaction is 0.0147 s-1.If the initial concentration of reactant is 0.178 M,what is the concentration of reactant after 30.0 seconds?

Accepted Answer

A)   8.72 × 105 M
B)   0.0645 M
C)   0.115 M
D)   0.0785 M
E)   0.643 M

Question 2

The decomposition of formic acid follows first-order kinetics. 
HCO2H(g) → CO2(g) + H2(g) 
The half-life for the reaction at 550°C is 24 seconds.How many seconds does it take for the formic acid concentration to decrease by 87.5%?

Accepted Answer

A)   24 s
B)   36 s
C)   48 s
D)   72 s
E)   96 s

Question 3

For the second-order reaction below,the rate constant of the reaction is 9.4 × 10-3 M-1s-1.How much time (in seconds) is required to decrease the concentration of A from 2.16 M to 0.40 M?  2 A→B rate =k[ A]22 \mathrm{~A} ightarrow \mathrm{B} \quad\quad\quad\quad\quad 	ext { rate }=k[\mathrm{~A}]^{2}2 A→B rate =k[ A]2

Accepted Answer

A)   2.0 × 101 s
B)   7.8 × 101 s
C)   1.8 × 102 s
D)   1.9 × 102 s
E)   2.2 × 102 s

Question 4

For the overall reaction A + 2B ? C
Which of the following mechanisms yields the correct overall chemical equation and is consistent with the rate equation below?
Rate = k[A]×[B]

Accepted Answer

A)    A+B⇌I (fast)  I+A→C (slow)  \begin{array}{l}\mathrm{A}+\mathrm{B} ightleftharpoons \mathrm{I} &	ext { (fast)  } \\mathrm{I}+\mathrm{A} ightarrow \mathrm{C} &	ext { (slow)  }\end{array}A+B⇌II+A→C​ (fast)   (slow)  ​ 
B)    A+B→I (slow)  I+B→C (fast)  \begin{array}{l}\mathrm{A}+\mathrm{B} ightarrow \mathrm{I} &	ext { (slow)  } \\mathrm{I}+\mathrm{B} ightarrow \mathrm{C} &	ext { (fast)  }\end{array}A+B→II+B→C​ (slow)   (fast)  ​ 
C)    2 B→I (slow)  A+I→C (fast)  \begin{array}{l}2 \mathrm{~B} ightarrow \mathrm{I} &	ext { (slow)  } \\mathrm{A}+\mathrm{I} ightarrow \mathrm{C} &	ext { (fast)  }\end{array}2 B→IA+I→C​ (slow)   (fast)  ​ 
D)    2 B⇌I (fast)  I+A→C (slow)  \begin{array}{l}2 \mathrm{~B} ightleftharpoons \mathrm{I}& 	ext { (fast)  } \\mathrm{I}+\mathrm{A} ightarrow \mathrm{C} &	ext { (slow)  }\end{array}2 B⇌II+A→C​ (fast)   (slow)  ​ 
E)   A+2 B⇌I (fast)  I+B→C+B (slow)  \begin{array}{l}\mathrm{A}+2 \mathrm{~B} ightleftharpoons \mathrm{I} &	ext { (fast)  } \\mathrm{I}+\mathrm{B} ightarrow \mathrm{C}+\mathrm{B} &	ext { (slow)  }\end{array}A+2 B⇌II+B→C+B​ (fast)   (slow)  ​

Question 5

For the reaction A + 2B ? C,the rate law is  Δ[C]Δt=k[ A]2×[B]\frac{\Delta[\mathrm{C}]}{\Delta t}=k[\mathrm{~A}]^{2} 	imes[\mathrm{B}]ΔtΔ[C]​=k[ A]2×[B]  . What are the units of the rate constant where time is measured in seconds?

Accepted Answer

A)    1 mol/L⋅s\frac{1}{\mathrm{~mol} / \mathrm{L} \cdot \mathrm{s}} mol/L⋅s1​ 
B)    1( mol/L) 2⋅s\frac{1}{(\mathrm{~mol} / \mathrm{L}) ^{2} \cdot \mathrm{s}}( mol/L) 2⋅s1​ 
C)    1 s\frac{1}{\mathrm{~s}} s1​ 
D)    (mol/L) 2 s\frac{(\mathrm{mol} / \mathrm{L}) ^{2}}{\mathrm{~s}} s(mol/L) 2​ 
E)    molL⋅s\frac{\mathrm{mol}}{\mathrm{L} \cdot \mathrm{s}}L⋅smol​

Question 6

The rate constant at 373 K for a certain reaction is 8.29 × 10−4 s−1 and the activation energy is 12.0 kJ/mole.What is the value of the constant,A,in the Arrhenius equation?

Accepted Answer

A)   0.00832 s−1
B)   0.0398 s−1
C)   0.120 s−1
D)   0.998 s−1
E)   25.1 s−1

Question 7

Which equation is used to calculate the half-life of the second-order equation below?  2 A→B rate =k[ A]22 \mathrm{~A} ightarrow \mathrm{B} \quad\quad\quad\quad\quad\quad\quad 	ext { rate }=k[\mathrm{~A}]^{2}2 A→B rate =k[ A]2

Accepted Answer

A)    t1/2=1k[A]0t_{1 / 2}=\frac{1}{k[A]_{0}}t1/2​=k[A]0​1​ 
B)    t1/2=ln⁡(2) k[A]0t_{1 / 2}=\frac{\ln (2) }{k[A]_{0}}t1/2​=k[A]0​ln(2) ​ 
C)    t1/2=ln⁡(2) kt_{1 / 2}=\frac{\ln (2) }{k}t1/2​=kln(2) ​ 
D)    t1/2=ln⁡(2) [A]0t_{1 / 2}=\frac{\ln (2) }{[A]_{0}}t1/2​=[A]0​ln(2) ​ 
E)    t1/2=k2[A]0t_{1 / 2}=\frac{k}{2[A]_{0}}t1/2​=2[A]0​k​

Question 8

For the second-order reaction below,the initial concentration of A is 1.00 M.If the concentration of A is reduced to 0.43 M after 75 seconds,what is the rate constant?  2 A→B rate =k[ A]22 \mathrm{~A} ightarrow \mathrm{B} \quad\quad\quad\quad\quad 	ext { rate }=k[\mathrm{~A}]^{2}2 A→B rate =k[ A]2

Accepted Answer

A)   5.2 × 10?4 L/mol?s
B)   5.7 × 10?3 L/mol?s
C)   7.6 × 10?3 L/mol?s
D)   1.1 × 10?2 L/mol?s
E)   1.8 × 10?2 L/mol?s

Question 9

The rate constant for the decomposition of cyclobutane is 2.08 × 10−2 s−1 at high temperatures. C4H8(g) → 2C2H4(g) 
How many seconds are required for an initial concentration of 0.100 M C4H8(g) to decrease to 0.0450 M?

Accepted Answer

A)   0.00114 s
B)   1.07 s
C)   2.64 s
D)   38.4 s
E)   874 s D

Question 10

Which equation is used to calculate the half-life of the zero-order equation below? A→2 B \mathrm{A} \rightarrow 2 \mathrm{~B} A→2 B \quad \quad \quad \quad \quad \quad \quad rate  =k =k =k

Accepted Answer

A)    t1/2=12kt_{1 / 2}=\frac{1}{2 k}t1/2​=2k1​ 
B)    t1/2=[A]0kt_{1 / 2}=\frac{[\mathrm{A}]_{0}}{k}t1/2​=k[A]0​​ 
C)    t1/2=[A]02kt_{1 / 2}=\frac{[A]_{0}}{2 k}t1/2​=2k[A]0​​ 
D)    t1/2=k[ A]0t_{1 / 2}=\frac{k}{[\mathrm{~A}]_{0}}t1/2​=[ A]0​k​ 
E)   t1/2 = k

Question 11

The elementary steps for the catalyzed decomposition for dinitrogen monoxide are shown below.Identify the catalyst. 
NO(g) + N2O(g) → N2(g) + NO2(g) 
2NO2(g) → 2NO(g) + O2(g)

Accepted Answer

A)   NO(g) 
B)   N2O(g) 
C)   N2(g) 
D)   NO2(g) 
E)   O2(g)

Question 12

For the first-order reaction below,the initial concentration of A is 0.240 M.If the concentration of A decreases to 0.0800 M after 21.8 hours,what is the half-life of the reaction?  A→B \mathrm{A} \rightarrow \mathrm{B} A→B \quad \quad \quad \quad \quad rate  =k[ A] =k[\mathrm{~A}] =k[ A]

Accepted Answer

A)   0.0504 hrs
B)   1.28 hrs
C)   7.26 hrs
D)   10.4 hrs
E)   13.8 hrs  E

Question 13

What did Henry Eyring develop that changed how scientists study rates of reactions?

Accepted Answer

A)   The catalyst model
B)   The transition-state model
C)   The liquid-state model
D)   The temperature dependence model
E)   The enzyme model

Question 14

For the second-order reaction below,the concentration of product B after 132 seconds is 0.0281 M.If the initial concentration of A is 0.932 M,what is the rate constant?  2 A→B rate =k[ A]22 \mathrm{~A} ightarrow \mathrm{B} \quad\quad\quad\quad\quad 	ext { rate }=k[\mathrm{~A}]^{2}2 A→B rate =k[ A]2

Accepted Answer

A)   1.43 × 10?5 L/mol?s
B)   4.71 × 10?4 L/mol?s
C)   5.22 × 10?4 L/mol?s
D)   6.63 × 10?3 L/mol?s
E)   96.4 L/mol?s

Question 15

Nitrogen dioxide reacts with carbon monoxide to produce nitrogen monoxide and carbon dioxide. 
 2NO2(g) ⇌NO3(g) +NO(g) (fast,equilibrium) NO3(g) +CO(g) →NO2(g) +CO2(g) (slow) \begin{array}{l}2 \mathrm{NO}_{2}(g)  ightleftharpoons \mathrm{NO}_{3}(g) +\mathrm{NO}(g)  &(fast, equilibrium) \\mathrm{NO}_{3}(g) +\mathrm{CO}(g)  ightarrow \mathrm{NO}_{2}(g) +\mathrm{CO}_{2}(g) &(slow)  \end{array}2NO2​(g) ⇌NO3​(g) +NO(g) NO3​(g) +CO(g) →NO2​(g) +CO2​(g) ​(fast,equilibrium) (slow) ​

What is a rate law that is consistent with the proposed mechanism?

Accepted Answer

A)   rate = k[NO2]2×[CO]× [NO]-1
B)   rate = k[NO2]2×[CO]
C)   rate = k[NO2]×[CO]
D)   rate = k[NO3]×[CO]
E)   rate = k[NO2]2

Question 16

At a high temperature,the first-order decomposition of N2O5(g) produces NO2(g) and O2(g) .If the initial concentration of 0.400 M N2O5(g) is reduced to 0.169 M after 118 seconds,what is the rate constant for the reaction?

Accepted Answer

A)   1.96 × 10−3 s−1
B)   2.29 × 10−3 s−1
C)   4.37 × 10−3 s−1
D)   7.30 × 10−3 s−1
E)   1.37 × 102 s−1

Question 17

A first-order reaction has a half-life of 4.54 seconds.How much time is required for the reactant to be reduced to 6.25% of its initial concentration?

Accepted Answer

A)   1.14 s
B)   9.08 s
C)   13.6 s
D)   18.2 s
E)   93.6 s

Question 18

The reaction A → B follows first-order kinetics with a half-life of 21.7 hours.If the concentration of A is 0.023 M after 48.0 hours,what is the initial concentration of A?

Accepted Answer

A)   0.0050 M
B)   0.051 M
C)   0.51 M
D)   0.11 M
E)   2.0 × 102 M

Question 19

The correct form of the Arrhenius equation is

Accepted Answer

A)   Ea = Ae?k/RT
B)    k=Ae−Ea/RTk=A e^{-E_{a} / R T}k=Ae−Ea​/RT 
C)    k=Ae−RT/Eak=A e^{-R T / E_{a}}k=Ae−RT/Ea​ 
D)   Ea = Aek/RT
E)   A = Eae?k/RT

Question 20

What is the half-life of a first-order reaction if the rate constant is 6.2 × 10-3 s-1?

Accepted Answer

A)   8.9 × 10-3 s
B)   0.097 s
C)   5.77 s
D)   1.1 × 102 s
E)   1.6 × 102 s D

Exam 11: Rate of Reaction

The rate constant of a first-order decomposition reaction is 0.0147 s^-1.If the initial concentration of reactant is 0.178 M,what is the concentration of reactant after 30.0 seconds?

Correct Answer
verified

The decomposition of formic acid follows first-order kinetics. HCO₂H(g) → CO₂(g) + H₂(g) The half-life for the reaction at 550°C is 24 seconds.How many seconds does it take for the formic acid concentration to decrease by 87.5%?

Correct Answer
verified

For the second-order reaction below,the rate constant of the reaction is 9.4 × 10^-3 M^-1s^-1.How much time (in seconds) is required to decrease the concentration of A from 2.16 M to 0.40 M? $2 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}$

Correct Answer
verified

For the overall reaction A + 2B ? C Which of the following mechanisms yields the correct overall chemical equation and is consistent with the rate equation below? Rate = k[A]×[B]

Correct Answer
verified

For the reaction A + 2B ? C,the rate law is $\frac{\Delta[\mathrm{C}]}{\Delta t}=k[\mathrm{~A}]^{2} \times[\mathrm{B}]$ . What are the units of the rate constant where time is measured in seconds?

Correct Answer
verified

The rate constant at 373 K for a certain reaction is 8.29 × 10−⁴ s−¹ and the activation energy is 12.0 kJ/mole.What is the value of the constant,A,in the Arrhenius equation?

Correct Answer
verified

Which equation is used to calculate the half-life of the second-order equation below? $2 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}$

Correct Answer
verified

For the second-order reaction below,the initial concentration of A is 1.00 M.If the concentration of A is reduced to 0.43 M after 75 seconds,what is the rate constant? $2 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}$

Correct Answer
verified

The rate constant for the decomposition of cyclobutane is 2.08 × 10−² s−¹ at high temperatures. C₄H₈(g) → 2C₂H₄(g) How many seconds are required for an initial concentration of 0.100 M C₄H₈(g) to decrease to 0.0450 M?

Correct Answer
verified
D

Which equation is used to calculate the half-life of the zero-order equation below? $\mathrm{A} \rightarrow 2 \mathrm{~B}$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ rate $=k$

Correct Answer
verified

The elementary steps for the catalyzed decomposition for dinitrogen monoxide are shown below.Identify the catalyst. NO(g) + N₂O(g) → N₂(g) + NO₂(g) 2NO₂(g) → 2NO(g) + O₂(g)

Correct Answer
verified

For the first-order reaction below,the initial concentration of A is 0.240 M.If the concentration of A decreases to 0.0800 M after 21.8 hours,what is the half-life of the reaction? $\mathrm{A} \rightarrow \mathrm{B}$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ rate $=k[\mathrm{~A}]$

Correct Answer
verified
E

What did Henry Eyring develop that changed how scientists study rates of reactions?

Correct Answer
verified

For the second-order reaction below,the concentration of product B after 132 seconds is 0.0281 M.If the initial concentration of A is 0.932 M,what is the rate constant? $2 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}$

Correct Answer
verified

Correct Answer
verified

At a high temperature,the first-order decomposition of N₂O₅(g) produces NO₂(g) and O₂(g) .If the initial concentration of 0.400 M N₂O₅(g) is reduced to 0.169 M after 118 seconds,what is the rate constant for the reaction?

Correct Answer
verified

A first-order reaction has a half-life of 4.54 seconds.How much time is required for the reactant to be reduced to 6.25% of its initial concentration?

Correct Answer
verified

The reaction A → B follows first-order kinetics with a half-life of 21.7 hours.If the concentration of A is 0.023 M after 48.0 hours,what is the initial concentration of A?

Correct Answer
verified

The correct form of the Arrhenius equation is

Correct Answer
verified

What is the half-life of a first-order reaction if the rate constant is 6.2 × 10^-3 s^-1?

Correct Answer
verified
D

Exam 11: Rate of Reaction

The rate constant of a first-order decomposition reaction is 0.0147 s-1.If the initial concentration of reactant is 0.178 M,what is the concentration of reactant after 30.0 seconds?

Correct AnswerverifiedShow Answer

The decomposition of formic acid follows first-order kinetics. HCO2H(g) → CO2(g) + H2(g) The half-life for the reaction at 550°C is 24 seconds.How many seconds does it take for the formic acid concentration to decrease by 87.5%?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

For the overall reaction A + 2B ? C Which of the following mechanisms yields the correct overall chemical equation and is consistent with the rate equation below? Rate = k[A]×[B]

Correct AnswerverifiedShow Answer

For the reaction A + 2B ? C,the rate law is Δ[C]Δt=k[ A]2×[B]\frac{\Delta[\mathrm{C}]}{\Delta t}=k[\mathrm{~A}]^{2} \times[\mathrm{B}]ΔtΔ[C]​=k[ A]2×[B] . What are the units of the rate constant where time is measured in seconds?

Correct AnswerverifiedShow Answer

The rate constant at 373 K for a certain reaction is 8.29 × 10−4 s−1 and the activation energy is 12.0 kJ/mole.What is the value of the constant,A,in the Arrhenius equation?

Correct AnswerverifiedShow Answer

Which equation is used to calculate the half-life of the second-order equation below? 2 A→B rate =k[ A]22 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}2 A→B rate =k[ A]2

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The rate constant for the decomposition of cyclobutane is 2.08 × 10−2 s−1 at high temperatures. C4H8(g) → 2C2H4(g) How many seconds are required for an initial concentration of 0.100 M C4H8(g) to decrease to 0.0450 M?

Correct AnswerverifiedD

Which equation is used to calculate the half-life of the zero-order equation below? A→2 B \mathrm{A} \rightarrow 2 \mathrm{~B} A→2 B \quad \quad \quad \quad \quad \quad \quad rate =k =k =k

Correct AnswerverifiedShow Answer

The elementary steps for the catalyzed decomposition for dinitrogen monoxide are shown below.Identify the catalyst. NO(g) + N2O(g) → N2(g) + NO2(g) 2NO2(g) → 2NO(g) + O2(g)

Correct AnswerverifiedShow Answer

For the first-order reaction below,the initial concentration of A is 0.240 M.If the concentration of A decreases to 0.0800 M after 21.8 hours,what is the half-life of the reaction? A→B \mathrm{A} \rightarrow \mathrm{B} A→B \quad \quad \quad \quad \quad rate =k[ A] =k[\mathrm{~A}] =k[ A]

Correct AnswerverifiedE

What did Henry Eyring develop that changed how scientists study rates of reactions?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

At a high temperature,the first-order decomposition of N2O5(g) produces NO2(g) and O2(g) .If the initial concentration of 0.400 M N2O5(g) is reduced to 0.169 M after 118 seconds,what is the rate constant for the reaction?

Correct AnswerverifiedShow Answer

A first-order reaction has a half-life of 4.54 seconds.How much time is required for the reactant to be reduced to 6.25% of its initial concentration?

Correct AnswerverifiedShow Answer

The reaction A → B follows first-order kinetics with a half-life of 21.7 hours.If the concentration of A is 0.023 M after 48.0 hours,what is the initial concentration of A?

Correct AnswerverifiedShow Answer

The correct form of the Arrhenius equation is

Correct AnswerverifiedShow Answer

What is the half-life of a first-order reaction if the rate constant is 6.2 × 10-3 s-1?

Correct AnswerverifiedD

The rate constant of a first-order decomposition reaction is 0.0147 s^-1.If the initial concentration of reactant is 0.178 M,what is the concentration of reactant after 30.0 seconds?

Correct Answer
verified

The decomposition of formic acid follows first-order kinetics. HCO₂H(g) → CO₂(g) + H₂(g) The half-life for the reaction at 550°C is 24 seconds.How many seconds does it take for the formic acid concentration to decrease by 87.5%?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

For the reaction A + 2B ? C,the rate law is $\frac{\Delta[\mathrm{C}]}{\Delta t}=k[\mathrm{~A}]^{2} \times[\mathrm{B}]$ . What are the units of the rate constant where time is measured in seconds?

Correct Answer
verified

The rate constant at 373 K for a certain reaction is 8.29 × 10−⁴ s−¹ and the activation energy is 12.0 kJ/mole.What is the value of the constant,A,in the Arrhenius equation?

Correct Answer
verified

Which equation is used to calculate the half-life of the second-order equation below? $2 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}$

Correct Answer
verified

Correct Answer
verified

The rate constant for the decomposition of cyclobutane is 2.08 × 10−² s−¹ at high temperatures. C₄H₈(g) → 2C₂H₄(g) How many seconds are required for an initial concentration of 0.100 M C₄H₈(g) to decrease to 0.0450 M?

Correct Answer
verified
D

Which equation is used to calculate the half-life of the zero-order equation below? $\mathrm{A} \rightarrow 2 \mathrm{~B}$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ rate $=k$

Correct Answer
verified

The elementary steps for the catalyzed decomposition for dinitrogen monoxide are shown below.Identify the catalyst. NO(g) + N₂O(g) → N₂(g) + NO₂(g) 2NO₂(g) → 2NO(g) + O₂(g)

Correct Answer
verified

For the first-order reaction below,the initial concentration of A is 0.240 M.If the concentration of A decreases to 0.0800 M after 21.8 hours,what is the half-life of the reaction? $\mathrm{A} \rightarrow \mathrm{B}$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ rate $=k[\mathrm{~A}]$

Correct Answer
verified
E

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

At a high temperature,the first-order decomposition of N₂O₅(g) produces NO₂(g) and O₂(g) .If the initial concentration of 0.400 M N₂O₅(g) is reduced to 0.169 M after 118 seconds,what is the rate constant for the reaction?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

What is the half-life of a first-order reaction if the rate constant is 6.2 × 10^-3 s^-1?

Correct Answer
verified
D