Question 1

A second-order reaction has a rate constant of 1.25 M-1.s-1.If the initial reactant concentration is 1.0 M,calculate the time required for 90% reaction.

Accepted Answer

A) 1.3 s 
B) 7.2 s 
C) 0.13 s 
D) 17 s 
E) 0.89 s 
A) 1.3 s 
B) 7.2 s 
C) 0.13 s 
D) 17 s 
E) 0.89 s B

Question 2

A reaction that has a very low activation energy

Accepted Answer

A) has a rate that is very sensitive to temperature. 
B) has a rate that does not change much with temperature. 
C) must be second order. 
D) gives a curved Arrhenius plot. 
E) must be first order. 
A) has a rate that is very sensitive to temperature. 
B) has a rate that does not change much with temperature. 
C) must be second order. 
D) gives a curved Arrhenius plot. 
E) must be first order. B

Question 3

What is the half-life of a reaction that has a rate constant of 280 s-1?

Accepted Answer

A) 194 s 
B) 3.6 ms 
C) 404 ms 
D) Because the concentration of reactant is not given,the calculation cannot be performed. 
E) 2.5 ms 
A) 194 s 
B) 3.6 ms 
C) 404 ms 
D) Because the concentration of reactant is not given,the calculation cannot be performed. 
E) 2.5 ms E

Question 4

Consider the reaction 
NOBr(g)$\rightarrow$ NO(g)+ ½Br2(g)
A plot of [NOBr]-1 vs t gives a straight line with a slope of 2.00 M-1.s-1.The order of the reaction and the rate constant,respectively,are

Accepted Answer

A) second-order and 0.500 M-1.s-1 
B) first-order and 2.00 s-1 
C) second-order and 2.00 M-1.s-1 
D) first-order and 0.241 s-1. 
E) second-order and 16.6 M-1.s-1 
A) second-order and 0.500 M-1.s-1 
B) first-order and 2.00 s-1 
C) second-order and 2.00 M-1.s-1 
D) first-order and 0.241 s-1. 
E) second-order and 16.6 M-1.s-1

Question 5

Given: 4Fe2+(aq)+ O2(aq)+ 2H2O(l)$\rightarrow$4Fe3+(aq)+ 4OH-(aq)
Rate = k[Fe2+][OH-]2[O2]
The overall order of the reaction and the order with respect to O2 are

Accepted Answer

A) 4 and 1. 
B) 5 and 1. 
C) 3 and 1. 
D) 4 and 2. 
E) 7 and 1. 
A) 4 and 1. 
B) 5 and 1. 
C) 3 and 1. 
D) 4 and 2. 
E) 7 and 1.

Question 6

Consider the reaction 2N2O(g)$\rightarrow$  2N2(g)+ O2(g)
Rate = k[N2O]
Calculate the time required for the concentration of N2O(g)to decrease from 0.75 M to 0.33 M.The rate constant for the reaction is k = 6.8 * 10-3 s-1.

Accepted Answer

A) 2.7 min 
B) 1.7 min 
C) 0.87 min 
D) 0.92 min 
E) 2.0 min 
A) 2.7 min 
B) 1.7 min 
C) 0.87 min 
D) 0.92 min 
E) 2.0 min

Question 7

The rate law for the following mechanism is ClO-(aq)+ H2O(l) →HOCl(aq)+ OH-(aq)
K,fast
I-(aq)+ HOCl(aq)$\rightarrow$ HOI(aq)+ Cl-(aq)
K1,slow
HOI(aq)+ OH-(aq)$\rightarrow$ OI-(aq)+ H2O(l)
K2,fast

Accepted Answer

A) rate = k1[I-][HOCl]. 
B) rate = k1K[ClO-][I-][OH-]. 
C) rate = k1K[ClO-][I-][OH-]-1.  
D) rate = k1k2K[ClO-][I-]. 
E) rate = k1K[ClO-][I-]. 
A) rate = k1[I-][HOCl]. 
B) rate = k1K[ClO-][I-][OH-]. 
C) rate = k1K[ClO-][I-][OH-]-1.  
D) rate = k1k2K[ClO-][I-]. 
E) rate = k1K[ClO-][I-].

Question 8

The rate law for a reaction can be determined from the coefficients in the overall reaction.

Accepted Answer

A) True 
 B)False

Question 9

A given compound decomposes with a half-life of 8.0 s and the half-life is independent of the concentration.How long does it take for the concentration to decrease to one-ninth of its initial value?

Accepted Answer

A) 32 s 
B) 25 s 
C) 72 s 
D) 64 s 
E) 3.6 s 
A) 32 s 
B) 25 s 
C) 72 s 
D) 64 s 
E) 3.6 s

Question 10

The fraction of molecules that collide with a kinetic energy equal to the activation energy for a reaction decreases rapidly with an increase in temperature.

Accepted Answer

A) True 
 B)False

Question 11

The reaction 2NO(g)+ 2H2(g)$\rightarrow$N2(g)+ 2H2O(g)
Is first order in H2 and second order in NO.Starting with equal concentrations of H2 and NO,the rate after 25% of the H2 has reacted is what percent of the initial rate?

Accepted Answer

A) 75.0% 
B) 42.2% 
C) 6.25% 
D) 56.3% 
E) 1.56% 
A) 75.0% 
B) 42.2% 
C) 6.25% 
D) 56.3% 
E) 1.56%

Question 12

The reaction 
3C + D $\rightarrow$ products
Has rate = k[D] and has a half-life of 1.29 s.If initially [D] = 0.820,what is the concentration of D after 2.55 s?

Accepted Answer

A) 0.21 
B) 0.12 
C) 0.56 
D) 0.28 
E) 0.41 
A) 0.21 
B) 0.12 
C) 0.56 
D) 0.28 
E) 0.41

Question 13

The reduction of M3+ by Cr2+ was studied with [Cr2+] 100 times the concentration of Cr2+.When [Cr2+] = 0.0050 M,the rate was 2.5 s-1.The rate constant for this reaction is

Accepted Answer

A) 1.3 M-1·s-1 
B) 0.013 M-1·s-1 
C) 5.0 M-1·s-1 
D) 500 M-1·s-1 
A) 1.3 M-1·s-1 
B) 0.013 M-1·s-1 
C) 5.0 M-1·s-1 
D) 500 M-1·s-1

Question 14

The reaction 2NO(g)+ 2H2(g)$\rightarrow$  N2(g)+ 2H2O(g)
Is first order in H2 and second order in NO.Starting with equal concentrations of H2 and NO,the rate after 50% of the H2 has reacted is what percent of the initial rate?

Accepted Answer

A) 18.8% 
B) 37.5% 
C) 25.0% 
D) 50.0% 
E) 12.5% 
A) 18.8% 
B) 37.5% 
C) 25.0% 
D) 50.0% 
E) 12.5%

Question 15

The rate of formation of oxygen in the reaction 2N2O5(g)$\rightarrow$ 4NO2(g)+ O2(g)
Is 2.28 (mol O2).L-1.s-1.What is the rate of formation of NO2?

Accepted Answer

A) 0.57 (mol NO2).L-1.s-1 
B) 9.12 (mol NO2).L-1.s-1 
C) 2.28 (mol NO2).L-1.s-1 
D) 1.14 (mol NO2).L-1.s-1 
E) 4.56 (mol NO2).L-1.s-1 
A) 0.57 (mol NO2).L-1.s-1 
B) 9.12 (mol NO2).L-1.s-1 
C) 2.28 (mol NO2).L-1.s-1 
D) 1.14 (mol NO2).L-1.s-1 
E) 4.56 (mol NO2).L-1.s-1

Question 16

A nonsteroidal anti-inflammatory drug is metabolized with a first-order rate constant of 3.25 day-1.What fraction of the drug remains in the body after 13.0 hr?

Accepted Answer

A) 0.172 
B) 0.0174 
C) 0.828 
D) 0.873 
E) 0.127 
A) 0.172 
B) 0.0174 
C) 0.828 
D) 0.873 
E) 0.127

Question 17

Given: 2A(g)+ B(g)$\rightarrow$ C(g)+ D(g)
When [A] = [B] = 0.10 M,the rate is 2.0 M.s-1; for [A] = [B] = 0.20,the rate is 8.0 M.s-1; and for [A] = 0.10 M,[B] = 0.20 M,the rate is 2.0 M.s-1.The rate law is

Accepted Answer

A) rate = k[A]. 
B) rate = k[B]2.  
C) rate = k[A][B]0.  
D) rate = k[A][B]. 
E) rate = k[A]2.  
A) rate = k[A]. 
B) rate = k[B]2.  
C) rate = k[A][B]0.  
D) rate = k[A][B]. 
E) rate = k[A]2.

Question 18

In the Michaelis-Menten mechanism of enzyme reaction,the Michaelis constant,KM,is

Accepted Answer

A) KM = k1/k2. 
B) KM = k1'/k2. 
C) KM = (k1' + k2)/k1. 
D) KM = k1' + k2. 
E) KM = k1/k1'. 
A) KM = k1/k2. 
B) KM = k1'/k2. 
C) KM = (k1' + k2)/k1. 
D) KM = k1' + k2. 
E) KM = k1/k1'.

Question 19

Consider the reaction for the dimerization of butadiene(g)at a certain temperature.
2C4H6(g)$\rightarrow$  C8H12(g)rate = k[C4H6]2.
When the initial concentration of butadiene is 0.500 M,the time required for 80% dimerization is measured at 11.4 s.What is the rate constant for the dimerization?

Accepted Answer

0.704 M<su

Question 20

A given first-order reaction has a rate constant of 0.00300 s-1.The time required for 85% reaction is

Accepted Answer

A) 632 s. 
B) 23.5 s. 
C) 275 s. 
D) 316 s. 
E) 54.2 s. 
A) 632 s. 
B) 23.5 s. 
C) 275 s. 
D) 316 s. 
E) 54.2 s.

A second-order reaction has a rate constant of 1.25 M^-1.s^-1.If the initial reactant concentration is 1.0 M,calculate the time required for 90% reaction.

A reaction that has a very low activation energy

What is the half-life of a reaction that has a rate constant of 280 s^-1?

Consider the reaction NOBr(g) $\rightarrow$ NO(g)+ ½Br₂(g) A plot of [NOBr]^-1 vs t gives a straight line with a slope of 2.00 M^-1.s^-1.The order of the reaction and the rate constant,respectively,are

Given: 4Fe²⁺(aq)+ O₂(aq)+ 2H₂O(l) $\rightarrow$ 4Fe³⁺(aq)+ 4OH^-(aq) Rate = k[Fe²⁺][OH^-]²[O₂] The overall order of the reaction and the order with respect to O₂ are

Consider the reaction 2N₂O(g) $\rightarrow$ 2N₂(g)+ O₂(g) Rate = k[N₂O] Calculate the time required for the concentration of N₂O(g)to decrease from 0.75 M to 0.33 M.The rate constant for the reaction is k = 6.8 * 10^-3 s^-1.

The rate law for the following mechanism is ClO^-(aq)+ H₂O(l) →HOCl(aq)+ OH^-(aq) K,fast I^-(aq)+ HOCl(aq) $\rightarrow$ HOI(aq)+ Cl^-(aq) K₁,slow HOI(aq)+ OH^-(aq) $\rightarrow$ OI^-(aq)+ H₂O(l) K₂,fast

The rate law for a reaction can be determined from the coefficients in the overall reaction.

A given compound decomposes with a half-life of 8.0 s and the half-life is independent of the concentration.How long does it take for the concentration to decrease to one-ninth of its initial value?

The fraction of molecules that collide with a kinetic energy equal to the activation energy for a reaction decreases rapidly with an increase in temperature.

The reaction 2NO(g)+ 2H₂(g) $\rightarrow$ N₂(g)+ 2H₂O(g) Is first order in H₂ and second order in NO.Starting with equal concentrations of H₂ and NO,the rate after 25% of the H₂ has reacted is what percent of the initial rate?

The reaction 3C + D $\rightarrow$ products Has rate = k[D] and has a half-life of 1.29 s.If initially [D] = 0.820,what is the concentration of D after 2.55 s?

The reduction of M³⁺ by Cr²⁺ was studied with [Cr²⁺] 100 times the concentration of Cr²⁺.When [Cr²⁺] = 0.0050 M,the rate was 2.5 s^-1.The rate constant for this reaction is

The reaction 2NO(g)+ 2H₂(g) $\rightarrow$ N₂(g)+ 2H₂O(g) Is first order in H₂ and second order in NO.Starting with equal concentrations of H₂ and NO,the rate after 50% of the H₂ has reacted is what percent of the initial rate?

The rate of formation of oxygen in the reaction 2N₂O₅(g) $\rightarrow$ 4NO₂(g)+ O₂(g) Is 2.28 (mol O₂).L^-1.s^-1.What is the rate of formation of NO₂?

A nonsteroidal anti-inflammatory drug is metabolized with a first-order rate constant of 3.25 day^-1.What fraction of the drug remains in the body after 13.0 hr?

Given: 2A(g)+ B(g) $\rightarrow$ C(g)+ D(g) When [A] = [B] = 0.10 M,the rate is 2.0 M.s^-1; for [A] = [B] = 0.20,the rate is 8.0 M.s^-1; and for [A] = 0.10 M,[B] = 0.20 M,the rate is 2.0 M.s^-1.The rate law is

In the Michaelis-Menten mechanism of enzyme reaction,the Michaelis constant,K_M,is

A given first-order reaction has a rate constant of 0.00300 s^-1.The time required for 85% reaction is

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Exam 15: Chemical Kinetics

A second-order reaction has a rate constant of 1.25 M-1.s-1.If the initial reactant concentration is 1.0 M,calculate the time required for 90% reaction.

A reaction that has a very low activation energy

What is the half-life of a reaction that has a rate constant of 280 s-1?

Consider the reaction NOBr(g) →\rightarrow→ NO(g)+ ½Br2(g) A plot of [NOBr]-1 vs t gives a straight line with a slope of 2.00 M-1.s-1.The order of the reaction and the rate constant,respectively,are

Given: 4Fe2+(aq)+ O2(aq)+ 2H2O(l) →\rightarrow→ 4Fe3+(aq)+ 4OH-(aq) Rate = k[Fe2+][OH-]2[O2] The overall order of the reaction and the order with respect to O2 are

Consider the reaction 2N2O(g) →\rightarrow→ 2N2(g)+ O2(g) Rate = k[N2O] Calculate the time required for the concentration of N2O(g)to decrease from 0.75 M to 0.33 M.The rate constant for the reaction is k = 6.8 * 10-3 s-1.

The rate law for the following mechanism is ClO-(aq)+ H2O(l) →HOCl(aq)+ OH-(aq) K,fast I-(aq)+ HOCl(aq) →\rightarrow→ HOI(aq)+ Cl-(aq) K1,slow HOI(aq)+ OH-(aq) →\rightarrow→ OI-(aq)+ H2O(l) K2,fast

The rate law for a reaction can be determined from the coefficients in the overall reaction.

A given compound decomposes with a half-life of 8.0 s and the half-life is independent of the concentration.How long does it take for the concentration to decrease to one-ninth of its initial value?

The fraction of molecules that collide with a kinetic energy equal to the activation energy for a reaction decreases rapidly with an increase in temperature.

The reaction 2NO(g)+ 2H2(g) →\rightarrow→ N2(g)+ 2H2O(g) Is first order in H2 and second order in NO.Starting with equal concentrations of H2 and NO,the rate after 25% of the H2 has reacted is what percent of the initial rate?

The reaction 3C + D →\rightarrow→ products Has rate = k[D] and has a half-life of 1.29 s.If initially [D] = 0.820,what is the concentration of D after 2.55 s?

The reduction of M3+ by Cr2+ was studied with [Cr2+] 100 times the concentration of Cr2+.When [Cr2+] = 0.0050 M,the rate was 2.5 s-1.The rate constant for this reaction is

The reaction 2NO(g)+ 2H2(g) →\rightarrow→ N2(g)+ 2H2O(g) Is first order in H2 and second order in NO.Starting with equal concentrations of H2 and NO,the rate after 50% of the H2 has reacted is what percent of the initial rate?

The rate of formation of oxygen in the reaction 2N2O5(g) →\rightarrow→ 4NO2(g)+ O2(g) Is 2.28 (mol O2).L-1.s-1.What is the rate of formation of NO2?

A nonsteroidal anti-inflammatory drug is metabolized with a first-order rate constant of 3.25 day-1.What fraction of the drug remains in the body after 13.0 hr?

Given: 2A(g)+ B(g) →\rightarrow→ C(g)+ D(g) When [A] = [B] = 0.10 M,the rate is 2.0 M.s-1; for [A] = [B] = 0.20,the rate is 8.0 M.s-1; and for [A] = 0.10 M,[B] = 0.20 M,the rate is 2.0 M.s-1.The rate law is

In the Michaelis-Menten mechanism of enzyme reaction,the Michaelis constant,KM,is

Consider the reaction for the dimerization of butadiene(g)at a certain temperature. 2C4H6(g) →\rightarrow→ C8H12(g)rate = k[C4H6]2. When the initial concentration of butadiene is 0.500 M,the time required for 80% dimerization is measured at 11.4 s.What is the rate constant for the dimerization?

A given first-order reaction has a rate constant of 0.00300 s-1.The time required for 85% reaction is

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A second-order reaction has a rate constant of 1.25 M^-1.s^-1.If the initial reactant concentration is 1.0 M,calculate the time required for 90% reaction.

What is the half-life of a reaction that has a rate constant of 280 s^-1?

Consider the reaction NOBr(g) $\rightarrow$ NO(g)+ ½Br₂(g) A plot of [NOBr]^-1 vs t gives a straight line with a slope of 2.00 M^-1.s^-1.The order of the reaction and the rate constant,respectively,are

Given: 4Fe²⁺(aq)+ O₂(aq)+ 2H₂O(l) $\rightarrow$ 4Fe³⁺(aq)+ 4OH^-(aq) Rate = k[Fe²⁺][OH^-]²[O₂] The overall order of the reaction and the order with respect to O₂ are

Consider the reaction 2N₂O(g) $\rightarrow$ 2N₂(g)+ O₂(g) Rate = k[N₂O] Calculate the time required for the concentration of N₂O(g)to decrease from 0.75 M to 0.33 M.The rate constant for the reaction is k = 6.8 * 10^-3 s^-1.

The rate law for the following mechanism is ClO^-(aq)+ H₂O(l) →HOCl(aq)+ OH^-(aq) K,fast I^-(aq)+ HOCl(aq) $\rightarrow$ HOI(aq)+ Cl^-(aq) K₁,slow HOI(aq)+ OH^-(aq) $\rightarrow$ OI^-(aq)+ H₂O(l) K₂,fast

The reaction 2NO(g)+ 2H₂(g) $\rightarrow$ N₂(g)+ 2H₂O(g) Is first order in H₂ and second order in NO.Starting with equal concentrations of H₂ and NO,the rate after 25% of the H₂ has reacted is what percent of the initial rate?

The reaction 3C + D $\rightarrow$ products Has rate = k[D] and has a half-life of 1.29 s.If initially [D] = 0.820,what is the concentration of D after 2.55 s?

The reduction of M³⁺ by Cr²⁺ was studied with [Cr²⁺] 100 times the concentration of Cr²⁺.When [Cr²⁺] = 0.0050 M,the rate was 2.5 s^-1.The rate constant for this reaction is

The reaction 2NO(g)+ 2H₂(g) $\rightarrow$ N₂(g)+ 2H₂O(g) Is first order in H₂ and second order in NO.Starting with equal concentrations of H₂ and NO,the rate after 50% of the H₂ has reacted is what percent of the initial rate?

The rate of formation of oxygen in the reaction 2N₂O₅(g) $\rightarrow$ 4NO₂(g)+ O₂(g) Is 2.28 (mol O₂).L^-1.s^-1.What is the rate of formation of NO₂?

A nonsteroidal anti-inflammatory drug is metabolized with a first-order rate constant of 3.25 day^-1.What fraction of the drug remains in the body after 13.0 hr?

Given: 2A(g)+ B(g) $\rightarrow$ C(g)+ D(g) When [A] = [B] = 0.10 M,the rate is 2.0 M.s^-1; for [A] = [B] = 0.20,the rate is 8.0 M.s^-1; and for [A] = 0.10 M,[B] = 0.20 M,the rate is 2.0 M.s^-1.The rate law is

In the Michaelis-Menten mechanism of enzyme reaction,the Michaelis constant,K_M,is

A given first-order reaction has a rate constant of 0.00300 s^-1.The time required for 85% reaction is