A possible mechanism for the reaction 2NO(g) + O2(g)$\rightarrow$2NO2(g) Is: 2NO(g) $f$ N2O2(g) K1,K1',Fast N2O2(g)+ O2(g)$\rightarrow$ 2NO2(g) K2,Slow Application of the steady-state approximation gives

A) [N2O2] = 0. B) k1[NO]2 - k2[N2O2][O2] = 0. C) [N2O2] = (k1/k2)[NO]2. D) k1[NO]2 - k1'[N2O2] -k2[N2O2][O2] = 0. E) [N2O2] = (k1/k1')[NO]2. A) [N2O2] = 0. B) k1[NO]2 - k2[N2O2][O2] = 0. C) [N2O2] = (k1/k2)[NO]2. D) k1[NO]2 - k1'[N2O2] -k2[N2O2][O2] = 0. E) [N2O2] = (k1/k1')[NO]2. D

Consider the mechanism NO2(g)+ F2(g)$\rightarrow$NO2F(g)+ F(g) K1 (slow) F(g)+ NO2(g)$\rightarrow$ NO2F(g) K2 (fast) Give the molecularity of the first step and any intermediates in the mechanism.

A) 2, and F(g) B) 2, and NO2F(g) C) 2, and NO2(g) D) 1, and no intermediate E) 2, and no intermediate A) 2, and F(g) B) 2, and NO2F(g) C) 2, and NO2(g) D) 1, and no intermediate E) 2, and no intermediate A

For the proposed mechanism A + X $f$ B k1,K-1 (fast) B $\rightarrow$ products k2 (slow) What is the rate law?

A) rate = (k1k-1)[A][X] B) rate = k2[B] C) rate = (k1/k2)[A] D) rate = (k1k2/ k-1)[A] E) rate = (k1k2/ k-1)[A][X] A) rate = (k1k-1)[A][X] B) rate = k2[B] C) rate = (k1/k2)[A] D) rate = (k1k2/ k-1)[A] E) rate = (k1k2/ k-1)[A][X]

Given: 2O3(g)$\rightarrow$3O2(g) Rate = k[O3]2[O2]-1 The overall order of the reaction and the order with respect to [O3] are

A) -1 and 3. B) 1 and 2. C) 0 and 1. D) 2 and 2. E) 3 and 2. A) -1 and 3. B) 1 and 2. C) 0 and 1. D) 2 and 2. E) 3 and 2.

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 propagation reactions in this mechanism are reactions"

A) 6. B) 1, 2, 3, and 6. C) 2 and 3. D) 1, 2, and 3. E) 2, 3, and 6. A) 6. B) 1, 2, 3, and 6. C) 2 and 3. D) 1, 2, and 3. E) 2, 3, and 6.

The reaction 2NO(g) + O2(g)$\rightarrow$ 2NO2(g) Has $\Delta$Hr$\omicron$ = -4 kJ.mol-1. A possible mechanism for this reaction is 2NO(g) Rapid equilibrium,K $f$ N2O2(g) N2O2(g)+O2(g)$\rightarrow$2NO2(g) Slow,K If the activation energy for the reverse reaction is 225 kJ.mol-1. What is the activation energy for the forward reaction?

A) Because an intermediate is involved, the forward activation energy cannot be calculated with the given information. B) 111 kJ.mol-1. C) 339 kJ.mol-1. D) 114 kJ.mol-1. E) 55.5 kJ.mol-1. A) Because an intermediate is involved, the forward activation energy cannot be calculated with the given information. B) 111 kJ.mol-1. C) 339 kJ.mol-1. D) 114 kJ.mol-1. E) 55.5 kJ.mol-1.

Consider the reaction below. 2A + B2 $\rightarrow$ 2AB Rate = k[A]2[B] Which of the following mechanisms is likely and consistent with the experimental rate law? 1.A + A + B2$\rightarrow$ 2AB 2.B2 $f$ 2B K,Fast A + B $\rightarrow$ AB k,Slow" 3.B2 $\rightarrow$ 2B k1,Slow A + B $\rightarrow$ AB k2,Fast" 4.2A $f$ A2 K,Fast B2 + A2 $\rightarrow$ 2AB k,Slow"

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

For the reaction cyclobutane(g) $\rightarrow$ 2ethylene(g)At 800 K,A plot of ln[cyclobutane] vs t gives a straight line with a slope of -1.6 s-1.Calculate the time needed for the concentration of cyclobutane to fall to 1/16 of its initial value.

A) 2.3 s B) 1.7 s C) 1.3 s D) 0.63 s E) 1.6 s A) 2.3 s B) 1.7 s C) 1.3 s D) 0.63 s E) 1.6 s

For the reaction S2O82-(aq) + 3I-(aq)$\rightarrow$2SO42-(aq)+ I3-(aq), Rate =k[S2O82-][I-].When the reaction is followed under pseudo-first-order conditions with [S2O82-] = 200 m M and [I-] = 1.5 m M, The rate constant was 1.82 s-1.The second order rate constant,K,For the reaction is

A) 1.21 * 103 M-1.s-1. B) 6.07 * 103 M-1.s-1. C) 9.10 M-1.s-1. D) 1.37 * 10-2 M-1.s-1. E) 1.82 M-1.s-1.. A) 1.21 * 103 M-1.s-1. B) 6.07 * 103 M-1.s-1. C) 9.10 M-1.s-1. D) 1.37 * 10-2 M-1.s-1. E) 1.82 M-1.s-1..

Exam 7: Kinetics

A possible mechanism for the reaction 2NO(g) + O₂(g) $\rightarrow$ 2NO₂(g) Is: 2NO(g) $f$ N₂O₂(g) K₁,K₁',Fast N₂O₂(g)+ O₂(g) $\rightarrow$ 2NO₂(g) K₂,Slow Application of the steady-state approximation gives

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Question 1

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Given: A $\rightarrow$ P rate = k[A] If 20% of A reacts in 5.12 min,Calculate the time required for 90% of A to react.

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Question 2

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Consider the mechanism NO₂(g)+ F₂(g) $\rightarrow$ NO₂F(g)+ F(g) K₁ (slow) F(g)+ NO₂(g) $\rightarrow$ NO₂F(g) K₂ (fast) Give the molecularity of the first step and any intermediates in the mechanism.

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Question 3

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Consider the reaction 2A $\rightarrow$ B,Rate = k[A]² If the rate of disappearance of A is followed,derive the experimental rate constant.

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Question 4

For the reaction cyclopropane(g) $\rightarrow$ propene(g)at 500^$\omicron$C,a plot of ln[cyclopropane] vs t gives a straight line with a slope of -0.00067 s^-¹.What is the order of this reaction and what is the rate constant?

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Question 5

Given: A + B $\rightarrow$ P rate = k[A][B] Which of the following is true?

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Question 6

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?

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Question 7

For the reaction Cyclopropane $\rightarrow$ propene A plot of ln[cyclopropane] vs time in seconds gives a straight line with slope -4.1 * 10^-³ s^-¹ at 550^$\omicron$C.What is the rate constant for this reaction?

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Question 8

For the proposed mechanism A + X $f$ B k₁,K_-1(fast) B $\rightarrow$ products k₂ (slow) What is the rate law?

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Question 9

Given: 2O₃(g) $\rightarrow$ 3O₂(g) Rate = k[O₃]²[O₂]^-¹ The overall order of the reaction and the order with respect to [O₃] are

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Question 10

A first-order reaction has a half-life of 1.10 s .If the initial concentration of reactant is 0.384 M,How long will it take for the reactant concentration to reach 0.00100 M?

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Question 11

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 propagation reactions in this mechanism are reactions"

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Question 12

The reaction 2NO(g) + O₂(g) $\rightarrow$ 2NO₂(g) Has $\Delta$ H_r^$\omicron$ = -4 kJ.mol^-¹. A possible mechanism for this reaction is 2NO(g) Rapid equilibrium,K $f$ N₂O₂(g) N₂O₂(g)+O₂(g) $\rightarrow$ 2NO₂(g) Slow,K If the activation energy for the reverse reaction is 225 kJ.mol^-¹. What is the activation energy for the forward reaction?

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Question 13

Consider the reaction below. 2A + B₂ $\rightarrow$ 2AB Rate = k[A]²[B] Which of the following mechanisms is likely and consistent with the experimental rate law? 1.A + A + B₂ $\rightarrow$ 2AB 2.B₂ $f$ 2B K,Fast A + B $\rightarrow$ AB k,Slow" 3.B₂ $\rightarrow$ 2B k₁,Slow A + B $\rightarrow$ AB k₂,Fast" 4.2A $f$ A₂ K,Fast B₂ + A₂ $\rightarrow$ 2AB k,Slow"

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Question 14

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

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Question 15

For the reaction cyclobutane(g) $\rightarrow$ 2ethylene(g)At 800 K,A plot of ln[cyclobutane] vs t gives a straight line with a slope of -1.6 s^-¹.Calculate the time needed for the concentration of cyclobutane to fall to 1/16 of its initial value.

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Question 16

The reaction 2A + B $\rightarrow$ D + E has the rate law,rate = a[A]²[B]/(b + c[A]) where a,b,and c are constants.The following mechanism has been proposed for this reaction. A + B k₁,k_-1 $f$ I I + A $\rightarrow$ D + E k₂ I is an unstable intermediate present in minute concentrations.Show that this mechanism leads to the observed rate law and evaluate the constantsa,b,and c in terms of the rate constants k₁,k_-1,and k₂.

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Question 17

For the elementary reaction A + 2B $\rightarrow$ products, rate = k[A][B].

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Question 18

The reaction profile for the reaction [(CN)₅CoOH₂]²^-(aq)+ SCN^-(aq) $\rightarrow$ [(CN)₅CoSCN]³^- + H₂O(l) is $The reaction profile for the reaction [(CN)5CoOH2]2-(aq)+ SCN-(aq) \rightarrow [(CN)5CoSCN]3- + H2O(l) is Identify the structure of B.What do A and C represent?$ Identify the structure of B.What do A and C represent?

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Question 19

For the reaction S₂O₈2^-(aq) + 3I^-(aq) $\rightarrow$ 2SO₄2^-(aq)+ I₃-(aq), Rate =k[S₂O₈2^-][I^-].When the reaction is followed under pseudo-first-order conditions with [S₂O₈2^-] = 200 m M and [I^-] = 1.5 m M, The rate constant was 1.82 s^-¹.The second order rate constant,K,For the reaction is

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Question 20

Showing 1 - 20 of 87

A possible mechanism for the reaction 2NO(g) + O₂(g) $\rightarrow$ 2NO₂(g) Is: 2NO(g) $f$ N₂O₂(g) K₁,K₁',Fast N₂O₂(g)+ O₂(g) $\rightarrow$ 2NO₂(g) K₂,Slow Application of the steady-state approximation gives

Given: A $\rightarrow$ P rate = k[A] If 20% of A reacts in 5.12 min,Calculate the time required for 90% of A to react.

Consider the mechanism NO₂(g)+ F₂(g) $\rightarrow$ NO₂F(g)+ F(g) K₁ (slow) F(g)+ NO₂(g) $\rightarrow$ NO₂F(g) K₂ (fast) Give the molecularity of the first step and any intermediates in the mechanism.

Consider the reaction 2A $\rightarrow$ B,Rate = k[A]² If the rate of disappearance of A is followed,derive the experimental rate constant.

For the reaction cyclopropane(g) $\rightarrow$ propene(g)at 500^$\omicron$C,a plot of ln[cyclopropane] vs t gives a straight line with a slope of -0.00067 s^-¹.What is the order of this reaction and what is the rate constant?

Given: A + B $\rightarrow$ P rate = k[A][B] Which of the following is true?

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?

For the reaction Cyclopropane $\rightarrow$ propene A plot of ln[cyclopropane] vs time in seconds gives a straight line with slope -4.1 * 10^-³ s^-¹ at 550^$\omicron$C.What is the rate constant for this reaction?

For the proposed mechanism A + X $f$ B k₁,K_-1(fast) B $\rightarrow$ products k₂ (slow) What is the rate law?

Given: 2O₃(g) $\rightarrow$ 3O₂(g) Rate = k[O₃]²[O₂]^-¹ The overall order of the reaction and the order with respect to [O₃] are

A first-order reaction has a half-life of 1.10 s .If the initial concentration of reactant is 0.384 M,How long will it take for the reactant concentration to reach 0.00100 M?

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

For the reaction cyclobutane(g) $\rightarrow$ 2ethylene(g)At 800 K,A plot of ln[cyclobutane] vs t gives a straight line with a slope of -1.6 s^-¹.Calculate the time needed for the concentration of cyclobutane to fall to 1/16 of its initial value.

For the elementary reaction A + 2B $\rightarrow$ products, rate = k[A][B].

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Exam 7: Kinetics

A possible mechanism for the reaction 2NO(g) + O2(g) →\rightarrow→ 2NO2(g) Is: 2NO(g) fff N2O2(g) K1,K1',Fast N2O2(g)+ O2(g) →\rightarrow→ 2NO2(g) K2,Slow Application of the steady-state approximation gives

Given: A →\rightarrow→ P rate = k[A] If 20% of A reacts in 5.12 min,Calculate the time required for 90% of A to react.

Consider the mechanism NO2(g)+ F2(g) →\rightarrow→ NO2F(g)+ F(g) K1 (slow) F(g)+ NO2(g) →\rightarrow→ NO2F(g) K2 (fast) Give the molecularity of the first step and any intermediates in the mechanism.

Consider the reaction 2A →\rightarrow→ B,Rate = k[A]2 If the rate of disappearance of A is followed,derive the experimental rate constant.

For the reaction cyclopropane(g) →\rightarrow→ propene(g)at 500 ο\omicronο C,a plot of ln[cyclopropane] vs t gives a straight line with a slope of -0.00067 s-1.What is the order of this reaction and what is the rate constant?

Given: A + B →\rightarrow→ P rate = k[A][B] Which of the following is true?

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?

For the reaction Cyclopropane →\rightarrow→ propene A plot of ln[cyclopropane] vs time in seconds gives a straight line with slope -4.1 * 10-3 s-1 at 550 ο\omicronο C.What is the rate constant for this reaction?

For the proposed mechanism A + X fff B k1,K-1 (fast) B →\rightarrow→ products k2 (slow) What is the rate law?

Given: 2O3(g) →\rightarrow→ 3O2(g) Rate = k[O3]2[O2]-1 The overall order of the reaction and the order with respect to [O3] are

A first-order reaction has a half-life of 1.10 s .If the initial concentration of reactant is 0.384 M,How long will it take for the reactant concentration to reach 0.00100 M?

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

For the reaction cyclobutane(g) →\rightarrow→ 2ethylene(g)At 800 K,A plot of ln[cyclobutane] vs t gives a straight line with a slope of -1.6 s-1.Calculate the time needed for the concentration of cyclobutane to fall to 1/16 of its initial value.

For the elementary reaction A + 2B →\rightarrow→ products, rate = k[A][B].

The reaction profile for the reaction [(CN)5CoOH2]2-(aq)+ SCN-(aq) →\rightarrow→ [(CN)5CoSCN]3- + H2O(l) is Identify the structure of B.What do A and C represent?

For the reaction S2O82-(aq) + 3I-(aq) →\rightarrow→ 2SO42-(aq)+ I3-(aq), Rate =k[S2O82-][I-].When the reaction is followed under pseudo-first-order conditions with [S2O82-] = 200 m M and [I-] = 1.5 m M, The rate constant was 1.82 s-1.The second order rate constant,K,For the reaction is

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A possible mechanism for the reaction 2NO(g) + O₂(g) $\rightarrow$ 2NO₂(g) Is: 2NO(g) $f$ N₂O₂(g) K₁,K₁',Fast N₂O₂(g)+ O₂(g) $\rightarrow$ 2NO₂(g) K₂,Slow Application of the steady-state approximation gives

Given: A $\rightarrow$ P rate = k[A] If 20% of A reacts in 5.12 min,Calculate the time required for 90% of A to react.

Consider the mechanism NO₂(g)+ F₂(g) $\rightarrow$ NO₂F(g)+ F(g) K₁ (slow) F(g)+ NO₂(g) $\rightarrow$ NO₂F(g) K₂ (fast) Give the molecularity of the first step and any intermediates in the mechanism.

Consider the reaction 2A $\rightarrow$ B,Rate = k[A]² If the rate of disappearance of A is followed,derive the experimental rate constant.

For the reaction cyclopropane(g) $\rightarrow$ propene(g)at 500^$\omicron$C,a plot of ln[cyclopropane] vs t gives a straight line with a slope of -0.00067 s^-¹.What is the order of this reaction and what is the rate constant?

Given: A + B $\rightarrow$ P rate = k[A][B] Which of the following is true?

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?

For the reaction Cyclopropane $\rightarrow$ propene A plot of ln[cyclopropane] vs time in seconds gives a straight line with slope -4.1 * 10^-³ s^-¹ at 550^$\omicron$C.What is the rate constant for this reaction?

For the proposed mechanism A + X $f$ B k₁,K_-1(fast) B $\rightarrow$ products k₂ (slow) What is the rate law?

Given: 2O₃(g) $\rightarrow$ 3O₂(g) Rate = k[O₃]²[O₂]^-¹ The overall order of the reaction and the order with respect to [O₃] are

For the reaction cyclobutane(g) $\rightarrow$ 2ethylene(g)At 800 K,A plot of ln[cyclobutane] vs t gives a straight line with a slope of -1.6 s^-¹.Calculate the time needed for the concentration of cyclobutane to fall to 1/16 of its initial value.

For the elementary reaction A + 2B $\rightarrow$ products, rate = k[A][B].