For the reaction: C2H4Br2 + 3 KI → C2H4 + 2 KBr + KI3,when the rate of disappearance of C2H4Br2 is 2.0 × 10-5 M/s,what is the rate of disappearance of KI?

A) 0.67 × 10-5 M/s B) 2.0 × 10-5 M/s C) 4.0 × 10-5 M/s D) 6.0 × 10-5 M/s E) 1.0 × 10-5 M/s A) 0.67 × 10-5 M/s B) 2.0 × 10-5 M/s C) 4.0 × 10-5 M/s D) 6.0 × 10-5 M/s E) 1.0 × 10-5 M/s

For the reaction: C2H4Br2 + 3 KI → C2H4 + 2 KBr + KI3 Initial rate data at 60 °C are: The rate law is ________.

A) rate = k[KI] B) rate = k[C2H4Br2] C) rate = k[KI]2 D) rate = k[KI][C2H4Br2] E) rate = k[KI][C2H4Br2]2 A) rate = k[KI] B) rate = k[C2H4Br2] C) rate = k[KI]2 D) rate = k[KI][C2H4Br2] E) rate = k[KI][C2H4Br2]2

For the reaction: 2 N2O5(g)→ 4 NO2(g)+ O2(g)the rate law is: = k[N2O5] At 300 K,the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol.What is the half-life at 310 K?

A) 2.49 × 104 s B) 9.51 × 104 s C) 9.51 × 106 s D) 6.57 × 103 s E) 1.87 × 10-1 s A) 2.49 × 104 s B) 9.51 × 104 s C) 9.51 × 106 s D) 6.57 × 103 s E) 1.87 × 10-1 s

What is the rate law for the following mechanism? N2O + NO → N2ONO (Slow) N2ONO → N2 + NO2 (Fast)

A) Rate = k[N2O] B) Rate = k[NO] C) Rate = k[N2O][NO] D) Rate = k[N2][NO2] E) Rate = k[N2ONO] A) Rate = k[N2O] B) Rate = k[NO] C) Rate = k[N2O][NO] D) Rate = k[N2][NO2] E) Rate = k[N2ONO]

For the reaction 2 HgCl2 + C2O42- → products,data are: The rate law is Rate = k[HgCl2]x[C2O42-]y. Thus:

A) x = 2,y = 1 B) x = 2,y = 2 C) x = 1,y = 2 D) x = 1,y = 1 E) x = 0,y = 2 A) x = 2,y = 1 B) x = 2,y = 2 C) x = 1,y = 2 D) x = 1,y = 1 E) x = 0,y = 2

Why is rate = k[HgCl2] 2[C2O42-] not the rate law for the following mechanism? 2 HgCl2 + C2O42- → 2 Cl- + 2 CO2 + Hg2Cl2 (overall reaction) HgCl2 + C2O42- ⇌ HgCl2C2O42- (fast) HgCl2C2O42- + C2O42- → Hg + 2 C2O4Cl2- (slow) Hg + HgCl2 → Hg2Cl2 (fast) 2 C2O4Cl2- → C2O42- + 2 Cl- + 2 CO2 (fast)

A) The rate law is not based on the slow step of the proposed mechanism. B) The steps do not add to the overall reaction. C) The rate law does not agree with the overall reaction. D) The exponents of HgCl2 and C2O42- are not equal. E) The first step is not the slow step. A) The rate law is not based on the slow step of the proposed mechanism. B) The steps do not add to the overall reaction. C) The rate law does not agree with the overall reaction. D) The exponents of HgCl2 and C2O42- are not equal. E) The first step is not the slow step.

Exam 20: Chemical Kinetics

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For the reaction: C₂H₄Br₂ + 3 KI → C₂H₄+ 2 KBr + KI₃,when the rate of disappearance of C₂H₄Br₂ is 2.0 × 10^-5 M/s,what is the rate of disappearance of KI?

(Multiple Choice)

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Question 41

The first-order reaction,2 N₂O(g)→ 2 N₂(g)+ O₂(g),has a rate constant equal to 0.76 s^-1 at 1000 K.How long will it take for the concentration of N₂O to decrease to 12% of its initial concentration?

(Multiple Choice)

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Question 42

For the reaction: C₂H₄Br₂ + 3 KI → C₂H₄ + 2 KBr + KI₃ Initial rate data at 60 °C are: The rate law is ________.

(Multiple Choice)

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Question 43

For the reaction: 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)the rate law is: = k[N₂O₅] At 300 K,the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol.What is the half-life at 310 K?

(Multiple Choice)

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Question 44

Which of the following statements is correct?

(Multiple Choice)

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Question 45

The first-order reaction,SO₂Cl₂ → SO₂ + Cl₂,has a rate constant equal to 2.20 × 10^-5 s^-1 at 593 K.What percentage of the initial amount of SO₂Cl₂ will remain after 6.00 hours?

(Multiple Choice)

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Question 46

In the Arrhenius equation,ln k = ^-^E_a/RT + ln A,the symbol A denotes the initial concentration of A.

(True/False)

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Question 47

For the reaction: A → Products concentration-time data are: What is the order of this reaction with respect to [A]?

(Multiple Choice)

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Question 48

The combustion of ethylene proceeds by the reaction (g)+ (g)→ (g)+ O(g) When the rate of disappearance of Is 0.28 mol L^-1 ,the rate of appearance of Is ________

(Multiple Choice)

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Question 49

What is the rate law for the following mechanism? N₂O + NO → N₂ONO (Slow) N₂ONO → N₂ + NO₂ (Fast)

(Multiple Choice)

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Question 50

Which statement is INCORRECT?

(Multiple Choice)

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Question 51

Calculate rate constant k for a first order reaction with a half-life of 75.0 min.

(Multiple Choice)

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Question 52

Given the following initial rate data,calculate the specific rate constant.

(Multiple Choice)

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Question 53

The correct units of the specific rate constant for a zero order reaction are ________.

(Multiple Choice)

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Question 54

For the reaction 2 HgCl₂ + C₂O₄^2- → products,data are: The rate law is Rate = k[HgCl₂]^x[C₂O₄^2-]^y. Thus:

(Multiple Choice)

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Question 55

The reaction A + B → C + D is second order in A and zero order in B.The value of k is 0.012 M^-1 min^-1.What is the rate of this reaction when [A] = 0.125 M and [B] = 0.435 M?

(Multiple Choice)

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Question 56

The rate data from a chemical reaction shows that doubling the concentration of A with the concentration of B remaining constant causes the rate to increase by a factor of four.What is the reaction order for [A]?

(Multiple Choice)

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Question 57

Why is rate = k[HgCl₂] ²[C₂O₄^2-] not the rate law for the following mechanism? 2 HgCl₂ + C₂O₄^2- → 2 Cl^- + 2 CO₂ + Hg₂Cl₂ (overall reaction) HgCl₂ + C₂O₄^2- ⇌ HgCl₂C₂O₄^2- (fast) HgCl₂C₂O₄^2- + C₂O₄^2- → Hg + 2 C₂O₄Cl^2- (slow) Hg + HgCl₂ → Hg₂Cl₂ (fast) 2 C₂O₄Cl^2- → C₂O₄^2- + 2 Cl^- + 2 CO₂ (fast)

(Multiple Choice)

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Question 58

A particular first-order reaction has a rate constant of 1.35 × At 25.0 °C.What is the magnitude of k at

(Multiple Choice)

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Question 59

If the half-life of a reaction depends on the concentration of the reactant,then the reaction cannot be ________ order.

(Multiple Choice)

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Question 60

Showing 41 - 60 of 124

Exam 20: Chemical Kinetics

For the reaction: C2H4Br2 + 3 KI → C2H4 + 2 KBr + KI3,when the rate of disappearance of C2H4Br2 is 2.0 × 10-5 M/s,what is the rate of disappearance of KI?

The first-order reaction,2 N2O(g)→ 2 N2(g)+ O2(g),has a rate constant equal to 0.76 s-1 at 1000 K.How long will it take for the concentration of N2O to decrease to 12% of its initial concentration?

For the reaction: C2H4Br2 + 3 KI → C2H4 + 2 KBr + KI3 Initial rate data at 60 °C are: The rate law is ________.

For the reaction: 2 N2O5(g)→ 4 NO2(g)+ O2(g)the rate law is: = k[N2O5] At 300 K,the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol.What is the half-life at 310 K?

Which of the following statements is correct?

The first-order reaction,SO2Cl2 → SO2 + Cl2,has a rate constant equal to 2.20 × 10-5 s-1 at 593 K.What percentage of the initial amount of SO2Cl2 will remain after 6.00 hours?

In the Arrhenius equation,ln k = -Ea/RT + ln A,the symbol A denotes the initial concentration of A.

For the reaction: A → Products concentration-time data are: What is the order of this reaction with respect to [A]?

The combustion of ethylene proceeds by the reaction (g)+ (g)→ (g)+ O(g) When the rate of disappearance of Is 0.28 mol L-1 ,the rate of appearance of Is ________

What is the rate law for the following mechanism? N2O + NO → N2ONO (Slow) N2ONO → N2 + NO2 (Fast)

Which statement is INCORRECT?

Calculate rate constant k for a first order reaction with a half-life of 75.0 min.

Given the following initial rate data,calculate the specific rate constant.

The correct units of the specific rate constant for a zero order reaction are ________.

For the reaction 2 HgCl2 + C2O42- → products,data are: The rate law is Rate = k[HgCl2]x[C2O42-]y. Thus:

The reaction A + B → C + D is second order in A and zero order in B.The value of k is 0.012 M-1 min-1.What is the rate of this reaction when [A] = 0.125 M and [B] = 0.435 M?

The rate data from a chemical reaction shows that doubling the concentration of A with the concentration of B remaining constant causes the rate to increase by a factor of four.What is the reaction order for [A]?

A particular first-order reaction has a rate constant of 1.35 × At 25.0 °C.What is the magnitude of k at

If the half-life of a reaction depends on the concentration of the reactant,then the reaction cannot be ________ order.

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For the reaction: C₂H₄Br₂ + 3 KI → C₂H₄+ 2 KBr + KI₃,when the rate of disappearance of C₂H₄Br₂ is 2.0 × 10^-5 M/s,what is the rate of disappearance of KI?

The first-order reaction,2 N₂O(g)→ 2 N₂(g)+ O₂(g),has a rate constant equal to 0.76 s^-1 at 1000 K.How long will it take for the concentration of N₂O to decrease to 12% of its initial concentration?

For the reaction: C₂H₄Br₂ + 3 KI → C₂H₄ + 2 KBr + KI₃ Initial rate data at 60 °C are: The rate law is ________.

For the reaction: 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)the rate law is: = k[N₂O₅] At 300 K,the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol.What is the half-life at 310 K?

The first-order reaction,SO₂Cl₂ → SO₂ + Cl₂,has a rate constant equal to 2.20 × 10^-5 s^-1 at 593 K.What percentage of the initial amount of SO₂Cl₂ will remain after 6.00 hours?

In the Arrhenius equation,ln k = ^-^E_a/RT + ln A,the symbol A denotes the initial concentration of A.

The combustion of ethylene proceeds by the reaction (g)+ (g)→ (g)+ O(g) When the rate of disappearance of Is 0.28 mol L^-1 ,the rate of appearance of Is ________

What is the rate law for the following mechanism? N₂O + NO → N₂ONO (Slow) N₂ONO → N₂ + NO₂ (Fast)

For the reaction 2 HgCl₂ + C₂O₄^2- → products,data are: The rate law is Rate = k[HgCl₂]^x[C₂O₄^2-]^y. Thus:

The reaction A + B → C + D is second order in A and zero order in B.The value of k is 0.012 M^-1 min^-1.What is the rate of this reaction when [A] = 0.125 M and [B] = 0.435 M?