The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N2O5(g)→ 4 NO2(g)+ O2(g) If the rate of appearance of O2 is equal to 2.40 mol/min at a particular moment,what is the rate of disappearance of N2O5 at that moment?

A) 0.600 mol/min B) 1.20 mol/min C) 4.80 mol/min D) 9.60 mol/min A) 0.600 mol/min B) 1.20 mol/min C) 4.80 mol/min D) 9.60 mol/min

The reaction below is first order in H2 and second order in NO.What is the rate law for this reaction? 2 H2(g)+ 2 NO(g)→ N2(g)+ 2 H2O(g)

A) Rate = 2k[H2][NO] B) Rate = k[H2][NO]2 C) Rate = k[H2]1/2[NO] D) Rate = 2k[H2]1/2[NO]1/2 A) Rate = 2k[H2][NO] B) Rate = k[H2][NO]2 C) Rate = k[H2]1/2[NO] D) Rate = 2k[H2]1/2[NO]1/2

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N2O5(g)→ 4 NO2(g)+ O2(g) If the rate of disappearance of N2O5 is equal to 1.40 mol/min at a particular moment,what is the rate of appearance of NO2 at that moment?

A) 0.700 mol/min B) 1.40 mol/min C) 2.80 mol/min D) 5.60 mol/min A) 0.700 mol/min B) 1.40 mol/min C) 2.80 mol/min D) 5.60 mol/min

Given the following hypothetical reaction: 2 E(g)+ F(g)+ G(g)→ products.If the rate law is: Rate = k[E]2[F]-1,what is the overall order of reaction?

A) zero B) one C) two D) one-fourth A) zero B) one C) two D) one-fourth

For the reaction shown below,what is the relationship between the rate of formation of Br2 and the rate of reaction of ClO2- over the same time period? ClO2-(aq)+ 4 Br-(aq)+ 4 H+(aq)→ Cl-(aq)+ 2 Br2(aq)+2 H2O(l)

A) rate of formation of Br2 = 2 × rate of reaction of ClO2- B) rate of formation of Br2 = 1/2 × rate of reaction of ClO2- C) rate of formation of Br2 = 4 x rate of reaction of ClO2- D) rate of formation of Br2 = 8 x rate of reaction of ClO2- A) rate of formation of Br2 = 2 × rate of reaction of ClO2- B) rate of formation of Br2 = 1/2 × rate of reaction of ClO2- C) rate of formation of Br2 = 4 x rate of reaction of ClO2- D) rate of formation of Br2 = 8 x rate of reaction of ClO2-

Hydrogen iodide decomposes at 800 K via a second-order process to produce hydrogen and iodine according to the following chemical equation. 2HI(g)→ H2(g)+ I2(g) At 800 K it takes 233 seconds for the initial concentration of HI to decrease from 5.75 × 10-2 M to 2.50 × 10-2 M.What is the rate constant for the reaction at this temperature?

A) 1.90 × 10-4 M-1s-1 B) 9.70 × 10-2 M-1s-1 C) 10.3 M-1s-1 D) 5.27 × 103 M-1s-1 A) 1.90 × 10-4 M-1s-1 B) 9.70 × 10-2 M-1s-1 C) 10.3 M-1s-1 D) 5.27 × 103 M-1s-1

The following set of data was obtained by the method of initial rates for the reaction: 2 HgCl2(aq)+ C2O42-(aq)→ 2 Cl-(aq)+ 2 CO2(g)+ Hg2Cl2(s) What is the value of the rate constant,k?

A) 1.4 × 10-8 1/M2∙s B) 1.3 × 10-7 1/M2∙s C) 1.4 × 10-5 1/M2∙s D) 1.3 × 10-4 1/M2∙s A) 1.4 × 10-8 1/M2∙s B) 1.3 × 10-7 1/M2∙s C) 1.4 × 10-5 1/M2∙s D) 1.3 × 10-4 1/M2∙s

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) 1.2 × 10-3 M B) 2.5 × 10-2 M C) 5.0 × 10-2 M D) 1.0 × 10-1 M A) 1.2 × 10-3 M B) 2.5 × 10-2 M C) 5.0 × 10-2 M D) 1.0 × 10-1 M

Exam 13: Chemical Kinetics

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 0.40 M?

(Multiple Choice)

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Question 21

A reaction has a rate constant,k = 1.2 × 10^-12 s^-1 at 273 K and k = 5.1 × 10^-7 s^-1 at 373 K has an activation energy,E_a = ________ kJ/mol.

(Short Answer)

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Question 22

Iodide and hypochlorite ion react in aqueous solution according to the reaction below: I^- + OCl^- → OI^- + Cl^- If the concentration of OH^- in the solution is doubled,the rate of the reaction is halved.What is the order of the reaction with respect to OH^-?

(Multiple Choice)

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Question 23

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g) If the rate of appearance of O₂ is equal to 2.40 mol/min at a particular moment,what is the rate of disappearance of N₂O₅ at that moment?

(Multiple Choice)

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Question 24

The reaction below is first order in H₂ and second order in NO.What is the rate law for this reaction? 2 H₂(g)+ 2 NO(g)→ N₂(g)+ 2 H₂O(g)

(Multiple Choice)

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Question 25

The reaction for the decomposition of dinitrogen monoxide gas to form an oxygen radical is: .If the activation energy is 250 kJ/mol and the frequency factor is 8.0 × 10¹¹ s^-1,what is the rate constant for the first-order reaction at 1000 K?

(Multiple Choice)

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Question 26

The first-order isomerization reaction: cyclopropane → propene,has a rate constant of 1.10 × 10^-4 s^-1 at 470°C and 5.70 × 10^-4 s^-1 at 500°C.What is the activation energy,E_a,for the reaction?

(Multiple Choice)

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Question 27

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g) If the rate of disappearance of N₂O₅ is equal to 1.40 mol/min at a particular moment,what is the rate of appearance of NO₂ at that moment?

(Multiple Choice)

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Question 28

Given the following hypothetical reaction: 2 E(g)+ F(g)+ G(g)→ products.If the rate law is: Rate = k[E]²[F]^-1,what is the overall order of reaction?

(Multiple Choice)

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Question 29

The reaction below is first order in H₂ and one-half order in Br₂.The rate law for this reaction is ________. H₂(g)+ Br₂(g)→ 2 HBr(g)

(Essay)

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Question 30

A gaseous compound,C,undergoes catalytic decomposition at an initial rate of 0.45 M/s when [C]_o = 3.0 × 10^-3 M and 0.45 M/s when [C]_o = 9.0 × 10^-3 M.Therefore,this is a ________ order reaction.

(Short Answer)

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Question 31

For the reaction shown below,what is the relationship between the rate of formation of Br₂ and the rate of reaction of ClO₂^-over the same time period? ClO₂^-(aq)+ 4 Br^-(aq)+ 4 H⁺(aq)→ Cl^-(aq)+ 2 Br₂(aq)+2 H₂O(l)

(Multiple Choice)

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Question 32

Hydrogen iodide decomposes at 800 K via a second-order process to produce hydrogen and iodine according to the following chemical equation. 2HI(g)→ H₂(g)+ I₂(g) At 800 K it takes 233 seconds for the initial concentration of HI to decrease from 5.75 × 10^-2 M to 2.50 × 10^-2 M.What is the rate constant for the reaction at this temperature?

(Multiple Choice)

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Question 33

The following reaction is second order in A and first order in B: A + B → Products Rate = k[A]²[B] What is the rate constant k of this reaction in vessel (b)relative to the rate constant k of this reaction in vessel (a)? Each vessel has the same volume.Shaded spheres represent A molecules,and unshaded spheres represent B molecules.

(Multiple Choice)

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Question 34

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 6.0% of its initial concentration?

(Multiple Choice)

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Question 35

Shown is a concentration versus time plot for a reaction involving gases A,B,and C. -Which equation best represents the reaction?

(Multiple Choice)

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Question 36

The reaction below is second order in ClO₂ and first order in OH^-.If the rate is expressed in M/s,the rate constant,k,has the units ________. 2 ClO₂(aq)+ 2 OH^-(aq)→ ClO₃^-(aq)+ ClO₂^-(aq)+ H₂O(l)

(Short Answer)

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Question 37

The first-order reaction,SO₂Cl₂ → SO₂ + Cl₂,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO₂Cl₂ to fall to 14.5% of its initial value?

(Multiple Choice)

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Question 38

The following set of data was obtained by the method of initial rates for the reaction: 2 HgCl₂(aq)+ C₂O₄^2-(aq)→ 2 Cl^-(aq)+ 2 CO₂(g)+ Hg₂Cl₂(s) What is the value of the rate constant,k?

(Multiple Choice)

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Question 39

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 40

Showing 21 - 40 of 190

Exam 13: Chemical Kinetics

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 0.40 M?

A reaction has a rate constant,k = 1.2 × 10-12 s-1 at 273 K and k = 5.1 × 10-7 s-1 at 373 K has an activation energy,Ea = ________ kJ/mol.

Iodide and hypochlorite ion react in aqueous solution according to the reaction below: I- + OCl- → OI- + Cl- If the concentration of OH- in the solution is doubled,the rate of the reaction is halved.What is the order of the reaction with respect to OH-?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N2O5(g)→ 4 NO2(g)+ O2(g) If the rate of appearance of O2 is equal to 2.40 mol/min at a particular moment,what is the rate of disappearance of N2O5 at that moment?

The reaction below is first order in H2 and second order in NO.What is the rate law for this reaction? 2 H2(g)+ 2 NO(g)→ N2(g)+ 2 H2O(g)

The reaction for the decomposition of dinitrogen monoxide gas to form an oxygen radical is: .If the activation energy is 250 kJ/mol and the frequency factor is 8.0 × 1011 s-1,what is the rate constant for the first-order reaction at 1000 K?

The first-order isomerization reaction: cyclopropane → propene,has a rate constant of 1.10 × 10-4 s-1 at 470°C and 5.70 × 10-4 s-1 at 500°C.What is the activation energy,Ea,for the reaction?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N2O5(g)→ 4 NO2(g)+ O2(g) If the rate of disappearance of N2O5 is equal to 1.40 mol/min at a particular moment,what is the rate of appearance of NO2 at that moment?

Given the following hypothetical reaction: 2 E(g)+ F(g)+ G(g)→ products.If the rate law is: Rate = k[E]2[F]-1,what is the overall order of reaction?

The reaction below is first order in H2 and one-half order in Br2.The rate law for this reaction is ________. H2(g)+ Br2(g)→ 2 HBr(g)

A gaseous compound,C,undergoes catalytic decomposition at an initial rate of 0.45 M/s when [C]o = 3.0 × 10-3 M and 0.45 M/s when [C]o = 9.0 × 10-3 M.Therefore,this is a ________ order reaction.

For the reaction shown below,what is the relationship between the rate of formation of Br2 and the rate of reaction of ClO2- over the same time period? ClO2-(aq)+ 4 Br-(aq)+ 4 H+(aq)→ Cl-(aq)+ 2 Br2(aq)+2 H2O(l)

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 6.0% of its initial concentration?

Shown is a concentration versus time plot for a reaction involving gases A,B,and C. -Which equation best represents the reaction?

The reaction below is second order in ClO2 and first order in OH-.If the rate is expressed in M/s,the rate constant,k,has the units ________. 2 ClO2(aq)+ 2 OH-(aq)→ ClO3-(aq)+ ClO2-(aq)+ H2O(l)

The first-order reaction,SO2Cl2 → SO2 + Cl2,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO2Cl2 to fall to 14.5% of its initial value?

The following set of data was obtained by the method of initial rates for the reaction: 2 HgCl2(aq)+ C2O42-(aq)→ 2 Cl-(aq)+ 2 CO2(g)+ Hg2Cl2(s) What is the value of the rate constant,k?

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?

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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 0.40 M?

A reaction has a rate constant,k = 1.2 × 10^-12 s^-1 at 273 K and k = 5.1 × 10^-7 s^-1 at 373 K has an activation energy,E_a = ________ kJ/mol.

Iodide and hypochlorite ion react in aqueous solution according to the reaction below: I^- + OCl^- → OI^- + Cl^- If the concentration of OH^- in the solution is doubled,the rate of the reaction is halved.What is the order of the reaction with respect to OH^-?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g) If the rate of appearance of O₂ is equal to 2.40 mol/min at a particular moment,what is the rate of disappearance of N₂O₅ at that moment?

The reaction below is first order in H₂ and second order in NO.What is the rate law for this reaction? 2 H₂(g)+ 2 NO(g)→ N₂(g)+ 2 H₂O(g)

The reaction for the decomposition of dinitrogen monoxide gas to form an oxygen radical is: .If the activation energy is 250 kJ/mol and the frequency factor is 8.0 × 10¹¹ s^-1,what is the rate constant for the first-order reaction at 1000 K?

The first-order isomerization reaction: cyclopropane → propene,has a rate constant of 1.10 × 10^-4 s^-1 at 470°C and 5.70 × 10^-4 s^-1 at 500°C.What is the activation energy,E_a,for the reaction?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g) If the rate of disappearance of N₂O₅ is equal to 1.40 mol/min at a particular moment,what is the rate of appearance of NO₂ at that moment?

Given the following hypothetical reaction: 2 E(g)+ F(g)+ G(g)→ products.If the rate law is: Rate = k[E]²[F]^-1,what is the overall order of reaction?

The reaction below is first order in H₂ and one-half order in Br₂.The rate law for this reaction is ________. H₂(g)+ Br₂(g)→ 2 HBr(g)

A gaseous compound,C,undergoes catalytic decomposition at an initial rate of 0.45 M/s when [C]_o = 3.0 × 10^-3 M and 0.45 M/s when [C]_o = 9.0 × 10^-3 M.Therefore,this is a ________ order reaction.

For the reaction shown below,what is the relationship between the rate of formation of Br₂ and the rate of reaction of ClO₂^-over the same time period? ClO₂^-(aq)+ 4 Br^-(aq)+ 4 H⁺(aq)→ Cl^-(aq)+ 2 Br₂(aq)+2 H₂O(l)

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 6.0% of its initial concentration?

The reaction below is second order in ClO₂ and first order in OH^-.If the rate is expressed in M/s,the rate constant,k,has the units ________. 2 ClO₂(aq)+ 2 OH^-(aq)→ ClO₃^-(aq)+ ClO₂^-(aq)+ H₂O(l)

The first-order reaction,SO₂Cl₂ → SO₂ + Cl₂,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO₂Cl₂ to fall to 14.5% of its initial value?

The following set of data was obtained by the method of initial rates for the reaction: 2 HgCl₂(aq)+ C₂O₄^2-(aq)→ 2 Cl^-(aq)+ 2 CO₂(g)+ Hg₂Cl₂(s) What is the value of the rate constant,k?

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?