Question 1

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.

Question 2

Consider the following mechanism for the production of phosgene.
Cl2 $\rightarrow$ Cl + Cl
Cl + CO $\rightarrow$ COCl
COCl + Cl $\rightarrow$ COCl2
The molecularity of the first and second elementary reactions is ____ and ____.

Accepted Answer

Question 3

Consider the reaction
2N2O5(g)$\rightarrow$ 4NO2(g)+ O2(g)
Rate = k[N2O5]
If the initial concentration of N2O5 is 0.80 M,The concentration after 5 half-lives is

Accepted Answer

A)  0.11 M. 
B)  0.025 M. 
C)  0.032 M. 
D)  0.16 M. 
E)  0.050 M. 
A)  0.11 M. 
B)  0.025 M. 
C)  0.032 M. 
D)  0.16 M. 
E)  0.050 M.

Question 4

If the rate of reaction increases by a factor of 2.3 when the concentration of reactant increases by a factor of 1.5, the order of the reaction with respect to this reactant is

Accepted Answer

A)  2. 
B)  1. 
C)  1.5. 
D)  4. 
E)  3. 
A)  2. 
B)  1. 
C)  1.5. 
D)  4. 
E)  3.

Question 5

A nonsteroidal anti-inflammatory drug is metabolized with a first-order rate constant of 3.25day-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 6

If the rate of reaction increases by a factor of 9.6 when the concentration of reactant increases by a factor of 3.1, the order of the reaction with respect to this reactant is

Accepted Answer

A)  1.5 
B)  3 
C)  4 
D)  2 
E)  1 
A)  1.5 
B)  3 
C)  4 
D)  2 
E)  1

Question 7

Consider the reaction
A + B $\rightarrow$ C + D rate = k[A]2
The time it takes for [A] to decrease from 1.0 to 0.50 M is the same as the time it takes for [A] to decrease from0.50 to 0.25 M.

Accepted Answer

A) True 
 B)False

Question 8

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 9

For a zero-order reaction,the rate constant has the same units as the rate of reaction.

Accepted Answer

A) True 
 B)False

Question 10

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 11

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.

Question 12

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 13

Given:
CH4(g)+ Cl2(g)$\rightarrow$CH3Cl(g)+ HCl(g)
The rate law for this elementary process is

Accepted Answer

A)  rate = k[Cl2]. 
B)  k[CH3Cl][HCl]. 
C)  rate = k[CH4][Cl2]. 
D)  rate = k[CH4]. 
E)  rate = k[CH4]2.  
A)  rate = k[Cl2]. 
B)  k[CH3Cl][HCl]. 
C)  rate = k[CH4][Cl2]. 
D)  rate = k[CH4]. 
E)  rate = k[CH4]2.

Question 14

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 15

The concentration-time curves for two sets of reactions, A/B and C/D,
Are:   
Which of the reactions are first order?

Accepted Answer

A)  B and D 
B)  A and B 
C)  C and D 
D)  A and C 
A)  B and D 
B)  A and B 
C)  C and D 
D)  A and C

Question 16

The HBr synthesis is thought to involve the following reactions:
1.Br2$\rightarrow$2Br.
2.Br. + H2 $\rightarrow$ HBr + H.
3.H. + Br2 $\rightarrow$ HBr + Br.
4.2Br. $\rightarrow$Br2
5.2H. $\rightarrow$H2
6.H. + Br. $\rightarrow$ HBr
The chain termination reactions in this mechanism are reactions"

Accepted Answer

A)  3, 4, and 5. 
B)  4 and 5. 
C)  4, 5, and 6. 
D)  6. 
E)  3 and 4. 
A)  3, 4, and 5. 
B)  4 and 5. 
C)  4, 5, and 6. 
D)  6. 
E)  3 and 4.

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

For the reaction A $\rightarrow$products,the following data were collected. $$\begin{array} { | l | l | l | l | l | l | } 
\hline \text { time, s } & 0 & 1 & 2 & 3 & 4 \
\hline [ \mathrm { A } ] . \mathrm { M } & 1.00 & 0.430 & 0.270 & 0.200 & 0.160 \
\hline
\end{array}$$ 
Determine the order of the reaction and calculate the rate constant.

Accepted Answer

second-order,
1.33 M

Question 19

A reaction has k = 8.39 M-1.s-1   .How long does it take for the reactant concentration to drop from 0.0840 M to 0.0220 M?

Accepted Answer

A)  5.42 s 
B)  2.00 s 
C)  1.42 s 
D)  8.39 s 
E)  4.00 s 
A)  5.42 s 
B)  2.00 s 
C)  1.42 s 
D)  8.39 s 
E)  4.00 s

Question 20

For the reaction cyclobutane(g) $\rightarrow$ 2ethylene(g)
At 800 K,The half-life is 0.43 s.Calculate the time needed for the concentration of cyclobutane to fall to 1/64 of its initial value.

Accepted Answer

A)  2.2 s 
B)  2.6 s 
C)  16 ms 
D)  0.38 s 
E)  0.43 s 
A)  2.2 s 
B)  2.6 s 
C)  16 ms 
D)  0.38 s 
E)  0.43 s

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

Consider the following mechanism for the production of phosgene. Cl₂ $\rightarrow$ Cl + Cl Cl + CO $\rightarrow$ COCl COCl + Cl $\rightarrow$ COCl₂ The molecularity of the first and second elementary reactions is and .

Consider the reaction 2N₂O₅(g) $\rightarrow$ 4NO₂(g)+ O₂(g) Rate = k[N₂O₅] If the initial concentration of N₂O₅ is 0.80 M,The concentration after 5 half-lives is

If the rate of reaction increases by a factor of 2.3 when the concentration of reactant increases by a factor of 1.5, the order of the reaction with respect to this reactant is

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

If the rate of reaction increases by a factor of 9.6 when the concentration of reactant increases by a factor of 3.1, the order of the reaction with respect to this reactant is

Consider the reaction A + B $\rightarrow$ C + D rate = k[A]² The time it takes for [A] to decrease from 1.0 to 0.50 M is the same as the time it takes for [A] to decrease from0.50 to 0.25 M.

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

For a zero-order reaction,the rate constant has the same units as the rate of reaction.

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?

A reaction that has a very low activation energy

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

Given: CH₄(g)+ Cl₂(g) $\rightarrow$ CH₃Cl(g)+ HCl(g) The rate law for this elementary process is

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 concentration-time curves for two sets of reactions, A/B and C/D, Are: Which of the reactions are first order?

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

For the reaction A $\rightarrow$ products,the following data were collected. time, s 0 1 2 3 4 []. 1.00 0.430 0.270 0.200 0.160 Determine the order of the reaction and calculate the rate constant.

A reaction has k = 8.39 M^-¹.s^-¹ .How long does it take for the reactant concentration to drop from 0.0840 M to 0.0220 M?

For the reaction cyclobutane(g) $\rightarrow$ 2ethylene(g) At 800 K,The half-life is 0.43 s.Calculate the time needed for the concentration of cyclobutane to fall to 1/64 of its initial value.

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Exam 7: Kinetics

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

Consider the following mechanism for the production of phosgene. Cl2 →\rightarrow→ Cl + Cl Cl + CO →\rightarrow→ COCl COCl + Cl →\rightarrow→ COCl2 The molecularity of the first and second elementary reactions is ____ and ____.

Consider the reaction 2N2O5(g) →\rightarrow→ 4NO2(g)+ O2(g) Rate = k[N2O5] If the initial concentration of N2O5 is 0.80 M,The concentration after 5 half-lives is

If the rate of reaction increases by a factor of 2.3 when the concentration of reactant increases by a factor of 1.5, the order of the reaction with respect to this reactant is

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

If the rate of reaction increases by a factor of 9.6 when the concentration of reactant increases by a factor of 3.1, the order of the reaction with respect to this reactant is

Consider the reaction A + B →\rightarrow→ C + D rate = k[A]2 The time it takes for [A] to decrease from 1.0 to 0.50 M is the same as the time it takes for [A] to decrease from0.50 to 0.25 M.

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

For a zero-order reaction,the rate constant has the same units as the rate of reaction.

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?

A reaction that has a very low activation energy

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

Given: CH4(g)+ Cl2(g) →\rightarrow→ CH3Cl(g)+ HCl(g) The rate law for this elementary process is

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 concentration-time curves for two sets of reactions, A/B and C/D, Are: Which of the reactions are first order?

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

For the reaction A →\rightarrow→ products,the following data were collected. time, s 0 1 2 3 4 []. 1.00 0.430 0.270 0.200 0.160 Determine the order of the reaction and calculate the rate constant.

A reaction has k = 8.39 M-1.s-1 .How long does it take for the reactant concentration to drop from 0.0840 M to 0.0220 M?

For the reaction cyclobutane(g) →\rightarrow→ 2ethylene(g) At 800 K,The half-life is 0.43 s.Calculate the time needed for the concentration of cyclobutane to fall to 1/64 of its initial value.

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

Consider the following mechanism for the production of phosgene. Cl₂ $\rightarrow$ Cl + Cl Cl + CO $\rightarrow$ COCl COCl + Cl $\rightarrow$ COCl₂ The molecularity of the first and second elementary reactions is and .

Consider the reaction 2N₂O₅(g) $\rightarrow$ 4NO₂(g)+ O₂(g) Rate = k[N₂O₅] If the initial concentration of N₂O₅ is 0.80 M,The concentration after 5 half-lives is

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

Consider the reaction A + B $\rightarrow$ C + D rate = k[A]² The time it takes for [A] to decrease from 1.0 to 0.50 M is the same as the time it takes for [A] to decrease from0.50 to 0.25 M.

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

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?

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

Given: CH₄(g)+ Cl₂(g) $\rightarrow$ CH₃Cl(g)+ HCl(g) The rate law for this elementary process is

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.

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

For the reaction A $\rightarrow$ products,the following data were collected. time, s 0 1 2 3 4 []. 1.00 0.430 0.270 0.200 0.160 Determine the order of the reaction and calculate the rate constant.

A reaction has k = 8.39 M^-¹.s^-¹ .How long does it take for the reactant concentration to drop from 0.0840 M to 0.0220 M?

For the reaction cyclobutane(g) $\rightarrow$ 2ethylene(g) At 800 K,The half-life is 0.43 s.Calculate the time needed for the concentration of cyclobutane to fall to 1/64 of its initial value.