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 O2.What is the half-life at 350 K?

A) 67.3 s B) 9.3 × 106 s C) 1.09 × 10-17 s D) 2.48 × 104 s E) 0.145 s A) 67.3 s B) 9.3 × 106 s C) 1.09 × 10-17 s D) 2.48 × 104 s E) 0.145 s

What is the rate constant at 305 K for the reaction: 2 N2O5 → 2 N2O4 + O2, If k = 3.46 × 10-5 s-1 at 298 K and Ea = 106 kJ/mol?

A) 2.4 × 10-5 s-1 B) 4.8 × 10-5 s-1 C) 6.0 × 10-5 s-1 D) 1.2 × 10-5 s-1 E) 9.2 × 10-5 s-1 A) 2.4 × 10-5 s-1 B) 4.8 × 10-5 s-1 C) 6.0 × 10-5 s-1 D) 1.2 × 10-5 s-1 E) 9.2 × 10-5 s-1

Nitrogen dioxide decomposes at 300 °C via a second-order process to produce nitrogen monoxide and oxygen according to the following chemical equation: 2 NO2(g)→ 2 NO(g)+ O2(g). A sample of NO2(g)is initially placed in a 2.50 L reaction vessel at 300 °C.If the half-life and the rate constant at 300 °C are 11 seconds and 0.54 L mol-1 s-1,respectively,how many moles of NO2 were in the original sample?

A) 0.17 mol B) 0.42 mol C) 5.9 mol D) 15 mol A) 0.17 mol B) 0.42 mol C) 5.9 mol D) 15 mol

For the first-order reaction,2 N2O(g)→ 2 N2(g)+ O2(g),what is the concentration of N2O after 3 half-lives if Mol of N2O is initially placed into a 1.00 L reaction vessel?

A) 1.6 × 10-2 mol L-1 B) 3.1 × 10-2 mol L-1 C) 6.2 × 10-2 mol L-1 D) 1.2 × 10-1 mol L-1 A) 1.6 × 10-2 mol L-1 B) 3.1 × 10-2 mol L-1 C) 6.2 × 10-2 mol L-1 D) 1.2 × 10-1 mol L-1

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00?

A) The rate will decrease by a factor of 1/25.0. B) The rate will decrease by a factor of 1/5.00. C) The rate will increase by a factor of 5.00. D) The rate will increase by a factor of 25.0. A) The rate will decrease by a factor of 1/25.0. B) The rate will decrease by a factor of 1/5.00. C) The rate will increase by a factor of 5.00. D) The rate will increase by a factor of 25.0.

For 2 NO + O2 → 2 NO2,initial rate data are: The rate law is Rate = k[NO][O2]y:

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

A) A theoretical equation that describes how the rate of reaction depends on the concentration of reactants. B) An experimentally determined equation that describes how the rate of reaction depends on the concentration of reactants. C) A theoretical equation that describes how the rate of reaction depends on temperature,orientation and number of collisions. D) An experimentally determined equation that describes how the rate of reaction depends on temperature,orientation and number of collisions. E) A statement that describes how the ratio of reaction depends on concentration of reactants developed from the balanced equation. A) A theoretical equation that describes how the rate of reaction depends on the concentration of reactants. B) An experimentally determined equation that describes how the rate of reaction depends on the concentration of reactants. C) A theoretical equation that describes how the rate of reaction depends on temperature,orientation and number of collisions. D) An experimentally determined equation that describes how the rate of reaction depends on temperature,orientation and number of collisions. E) A statement that describes how the ratio of reaction depends on concentration of reactants developed from the balanced equation.

Exam 20: Chemical Kinetics

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 O₂.What is the half-life at 350 K?

(Multiple Choice)

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Question 101

What is the rate constant at 305 K for the reaction: 2 N₂O₅ → 2 N₂O₄ + O₂, If k = 3.46 × 10^-5 s^-1 at 298 K and E_a = 106 kJ/mol?

(Multiple Choice)

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Question 102

If a catalyst is added to a reaction: I.the value of k is increased II.the value of k is decreased III.the rate is increased IV.the rate is decreased V.neither rate nor the constant are changed,only the order

(Multiple Choice)

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Question 103

Which of the following has no effect on the rate of a reaction?

(Multiple Choice)

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Question 104

Nitrogen dioxide decomposes at 300 °C via a second-order process to produce nitrogen monoxide and oxygen according to the following chemical equation: 2 NO₂(g)→ 2 NO(g)+ O₂(g). A sample of NO₂(g)is initially placed in a 2.50 L reaction vessel at 300 °C.If the half-life and the rate constant at 300 °C are 11 seconds and 0.54 L mol^-1 s^-1,respectively,how many moles of NO₂ were in the original sample?

(Multiple Choice)

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Question 105

For the second-order reaction A → products,the following data are obtained: [A] = 1.512 M,t = 0 min [A] = 1.490 M,t = 1.0 min [A] = 1.469 M,t = 2.0 min What is the initial rate of the reaction in the experiment?

(Multiple Choice)

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Question 106

For the reaction: 2 NO₂(g)→ 2 NO(g)+ O₂(g)concentration-time data are: What is the order of the reaction with respect to [NO₂]?

(Multiple Choice)

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Question 107

For the first-order reaction,2 N₂O(g)→ 2 N₂(g)+ O₂(g),what is the concentration of N₂O after 3 half-lives if Mol of N₂O is initially placed into a 1.00 L reaction vessel?

(Multiple Choice)

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Question 108

Which of the following statements is true about the reaction 2 A → B + C which is first order in A and first order overall?

(Multiple Choice)

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Question 109

Substance A decomposes by a first-order reaction.Starting initially with [A] = 2.00 M,after 150 min [A] = 0.50 M.For this reaction what is ?

(Multiple Choice)

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Question 110

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00?

(Multiple Choice)

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Question 111

Decomposes in the gas phase by the reaction The reaction is first order in And the rate constant is 3.0 × At 600 K.A vessel is charged with 2.4 atm of At 600 K.The partial pressure of At Is ________ atm.

(Multiple Choice)

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Question 112

For 2 NO + O₂ → 2 NO₂,initial rate data are: The rate law is Rate = k[NO][O₂]^y:

(Multiple Choice)

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Question 113

If increasing the concentration of A in a chemical reaction causes no increase in the rate of the reaction,then we may say the reaction rate is first order in [A].

(True/False)

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Question 114

Define rate law.

(Multiple Choice)

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Question 115

Which of the following is FALSE for a second order reaction?

(Multiple Choice)

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Question 116

Choose the INCORRECT answer.The rate of a chemical reaction:

(Multiple Choice)

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Question 117

In aqueous solution,hypobromite ion,BrO^-,reacts to produce bromate ion,BrO₃^-,and bromide ion,Br^-,according to the following chemical equation: A plot of 1/[BrO^-] vs.time is linear and the slope is equal to 0.056 L mol^-1s^-1.If the initial concentration of BrO^- is 0.80 mol L^-1,how long will it take one-half of the BrO^-ion to react?

(Multiple Choice)

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Question 118

If the half-life of a reactant is independent of its initial concentration,the reaction order is 0.

(True/False)

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Question 119

The isomerization reaction,CH₃NC → CH₃CN,is first order and the rate constant is equal to 0.46 s^-1 at 600 K.What is the concentration of CH₃NC after 0.20 minutes if the initial concentration is 0.30 mol L^-1?

(Multiple Choice)

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Question 120

Showing 101 - 120 of 124

Exam 20: Chemical Kinetics

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 O2.What is the half-life at 350 K?

What is the rate constant at 305 K for the reaction: 2 N2O5 → 2 N2O4 + O2, If k = 3.46 × 10-5 s-1 at 298 K and Ea = 106 kJ/mol?

If a catalyst is added to a reaction: I.the value of k is increased II.the value of k is decreased III.the rate is increased IV.the rate is decreased V.neither rate nor the constant are changed,only the order

Which of the following has no effect on the rate of a reaction?

For the second-order reaction A → products,the following data are obtained: [A] = 1.512 M,t = 0 min [A] = 1.490 M,t = 1.0 min [A] = 1.469 M,t = 2.0 min What is the initial rate of the reaction in the experiment?

For the reaction: 2 NO2(g)→ 2 NO(g)+ O2(g)concentration-time data are: What is the order of the reaction with respect to [NO2]?

For the first-order reaction,2 N2O(g)→ 2 N2(g)+ O2(g),what is the concentration of N2O after 3 half-lives if Mol of N2O is initially placed into a 1.00 L reaction vessel?

Which of the following statements is true about the reaction 2 A → B + C which is first order in A and first order overall?

Substance A decomposes by a first-order reaction.Starting initially with [A] = 2.00 M,after 150 min [A] = 0.50 M.For this reaction what is ?

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00?

Decomposes in the gas phase by the reaction The reaction is first order in And the rate constant is 3.0 × At 600 K.A vessel is charged with 2.4 atm of At 600 K.The partial pressure of At Is ________ atm.

For 2 NO + O2 → 2 NO2,initial rate data are: The rate law is Rate = k[NO][O2]y:

If increasing the concentration of A in a chemical reaction causes no increase in the rate of the reaction,then we may say the reaction rate is first order in [A].

Define rate law.

Which of the following is FALSE for a second order reaction?

Choose the INCORRECT answer.The rate of a chemical reaction:

If the half-life of a reactant is independent of its initial concentration,the reaction order is 0.

The isomerization reaction,CH3NC → CH3CN,is first order and the rate constant is equal to 0.46 s-1 at 600 K.What is the concentration of CH3NC after 0.20 minutes if the initial concentration is 0.30 mol L-1?

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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 O₂.What is the half-life at 350 K?

What is the rate constant at 305 K for the reaction: 2 N₂O₅ → 2 N₂O₄ + O₂, If k = 3.46 × 10^-5 s^-1 at 298 K and E_a = 106 kJ/mol?

For the reaction: 2 NO₂(g)→ 2 NO(g)+ O₂(g)concentration-time data are: What is the order of the reaction with respect to [NO₂]?

For the first-order reaction,2 N₂O(g)→ 2 N₂(g)+ O₂(g),what is the concentration of N₂O after 3 half-lives if Mol of N₂O is initially placed into a 1.00 L reaction vessel?

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00?

For 2 NO + O₂ → 2 NO₂,initial rate data are: The rate law is Rate = k[NO][O₂]^y:

The isomerization reaction,CH₃NC → CH₃CN,is first order and the rate constant is equal to 0.46 s^-1 at 600 K.What is the concentration of CH₃NC after 0.20 minutes if the initial concentration is 0.30 mol L^-1?