The half life of the reaction shown below is found not to depend on the concentration of H2O2(aq). 2 H2O2(aq)→ 2 H2O(l)+ O2(g) What is the order of this reaction?

A) zeroth B) first C) second D) third A) zeroth B) first C) second D) third

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 142 seconds for the initial concentration of HI to decrease from 6.75 × 10-2 M to 3.50 × 10-2 M.What is the rate constant for the reaction at this temperature?

A) 5)12 × 10- 4 M-1s-1 B) 9)69 × 10-2 M-1s-1 C) 10.3 M-1s-1 D) 1)95 × 103 M-1s-1 A) 5)12 × 10- 4 M-1s-1 B) 9)69 × 10-2 M-1s-1 C) 10.3 M-1s-1 D) 1)95 × 103 M-1s-1

Consider a reaction that occurs by the following one-step mechanism: AS1U1B12S1U1B0 + BS1U1B12S1U1B0 → 2 AB The potential energy profile for this reaction is shown below. -What is the species present at reaction stage 1?

A) an intermediate B) a product C) a reactant D) a transition state A) an intermediate B) a product C) a reactant D) a transition state

The hydrolysis of tert-butyl chloride is given in the reaction below: (CH3)3CCl(aq)+ H2O(l)→ (CH3)3COH(aq)+ H+(aq)+ Cl-(aq) If the rate law is: Rate = k[(CH3)3CCl],what is the order of the reaction with respect to water?

A) zero B) first C) second D) third A) zero B) first C) second D) third

The relative initial rates of the reaction AS1U1B12S1U1B0 + BS1U1B12S1U1B0 → products in vessels (a)-(d)are 1:1:4:4.Unshaded spheres represent AS1U1B12S1U1B0 molecules,and shaded spheres represent BS1U1B12S1U1B0 molecules present at the beginning of the reaction. -What is the overall order of reaction?

A) 0 B) 1 C) 2 D) 3 A) 0 B) 1 C) 2 D) 3

The reaction for the decomposition of dinitrogen monoxide gas to form an oxygen radical is: N2O(g) $\rarr$ N2(g)+ O(g).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?

A) 1)1 × 10-3 s-1 B) 7)0 × 10-2 s-1 C) 1)6 × 1013 s-1 D) 9)1 × 1024 s-1 A) 1)1 × 10-3 s-1 B) 7)0 × 10-2 s-1 C) 1)6 × 1013 s-1 D) 9)1 × 1024 s-1

The second-order reaction,2 Mn(CO)5 → Mn2(CO)10 has a rate constant equal to 3.0 × 109 M-1s-1 at 25°C.If the initial concentration of Mn(CO)5 is 1.0 × 10-5 M,how long will it take for 90.% of the reactant to disappear?

A) 3)3 × 10-16 s B) 3)7 × 10-15 s C) 3)0 × 10-4 s D) 3)0 × 103 s A) 3)3 × 10-16 s B) 3)7 × 10-15 s C) 3)0 × 10-4 s D) 3)0 × 103 s

A concentration-time study of the gas phase reaction 2 A3 → 3 A2 produced the data in the table below. Time (s)[A3] (M)[A2] (M) 0 4)00 × 10-4 0 10 2.00 × 10-4 3.00 × 10-4 20 1.00 × 10-4 4.50 × 10-4 30 5.00 × 10-5 ? What is the average rate of formation of A2 in the time interval 20-30 seconds?

A) 6)00 × 10-4 M/s B) 5)25 × 10-5 M/s C) 7)50 × 10-6 M/s D) 6)00 × 10-6 M/s A) 6)00 × 10-4 M/s B) 5)25 × 10-5 M/s C) 7)50 × 10-6 M/s D) 6)00 × 10-6 M/s

Exam 12: Chemical Kinetics

The half life of the reaction shown below is found not to depend on the concentration of H₂O₂(aq). 2 H₂O₂(aq)→ 2 H₂O(l)+ O₂(g) What is the order of this reaction?

(Multiple Choice)

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Question 41

The reaction below is second order in ClO₂ and first order in OH^-.When the concentration of ClO₂ is 0.020 M and the concentration of OH^- is 0.10 M,the initial rate of reaction is 8.00 × 10^-4 M/s.What is the rate constant,k,for this reaction? 2 ClO₂(aq)+ 2 OH^-(aq)→ ClO₃^-(aq)+ ClO₂^-(aq)+ H₂O(l)

(Short Answer)

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Question 42

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 142 seconds for the initial concentration of HI to decrease from 6.75 × 10^-2 M to 3.50 × 10^-2 M.What is the rate constant for the reaction at this temperature?

(Multiple Choice)

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Question 43

For the reaction shown below,if the rate of formation of Br₂ is 1.2 × 10^-6 M/s,over the same time period the rate of consumption of H⁺ is ________ M/s. ClO₂^-(aq)+ 4 Br^-(aq)+ 4 H⁺(aq)→ Cl^-(aq)+ 2 Br₂(aq)+2 H₂O(l)

(Short Answer)

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Question 44

Consider a reaction that occurs by the following one-step mechanism: A₂ + B₂ → 2 AB The potential energy profile for this reaction is shown below. -What is the species present at reaction stage 1?

(Multiple Choice)

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Question 45

For the reaction shown below,if the rate of formation of O₂ is 6.0 × 10^-6M/s,the rate of decomposition of N₂O₅ over the same time interval is ________. 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)

(Short Answer)

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Question 46

A reaction has the rate law Rate = k[NO]²[H₂].If the concentration of NO is reduced by 1/3,the rate of reaction will be (increased,decreased)by .

(Short Answer)

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Question 47

The hydrolysis of tert-butyl chloride is given in the reaction below: (CH₃)₃CCl(aq)+ H₂O(l)→ (CH₃)₃COH(aq)+ H⁺(aq)+ Cl^-(aq) If the rate law is: Rate = k[(CH₃)₃CCl],what is the order of the reaction with respect to water?

(Multiple Choice)

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Question 48

The relative initial rates of the reaction A₂ + B₂ → products in vessels (a)-(d)are 1:1:4:4.Unshaded spheres represent A₂ molecules,and shaded spheres represent B₂ molecules present at the beginning of the reaction. -What is the overall order of reaction?

(Multiple Choice)

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Question 49

The reaction for the decomposition of dinitrogen monoxide gas to form an oxygen radical is: N₂O(g) $\rarr$ N₂(g)+ O(g).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 50

Consider the first-order reaction A → B in which A molecules (unshaded spheres)are converted to B molecules (shaded spheres).Given the following pictures at t = 0 seconds and t = 100 seconds,which picture represents the number of A and B molecules remaining at 200 seconds?

(Multiple Choice)

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Question 51

The second-order reaction,2 Mn(CO)₅ → Mn₂(CO)₁₀ has a rate constant equal to 3.0 × 10⁹ M^-1s^-1 at 25°C.If the initial concentration of Mn(CO)₅ is 1.0 × 10^-5 M,how long will it take for 90.% of the reactant to disappear?

(Multiple Choice)

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Question 52

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 0.10 M?

(Multiple Choice)

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Question 53

The decomposition of cyclopropane,was observed at 500°C and its concentration was monitored as a function of time.The data set is given below.What is the order of the reaction with respect to cyclopropane?

(Multiple Choice)

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Question 54

The decay curve shown below approximates the decay of cobalt-60.What is the approximate half-life of cobalt-60?

(Multiple Choice)

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Question 55

Which of the following statements are true about reaction mechanisms? I.A rate law can be written from the molecularity of the slowest elementary step. II.The final rate law can include intermediates. III.The rate of the reaction is dependent on the fastest step in the mechanism. IV.A mechanism can never be proven to be the correct pathway for a reaction.

(Multiple Choice)

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Question 56

The following reaction is first order in A and first order in B: A + B → Products Rate = k[A][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 57

Acetaldehyde decomposes at 750 K: CH₃CHO → CO + CH₄.The reaction is first order in acetaldehyde and the half-life of the reaction is found to be 530 seconds.What is the rate constant for the reaction at this temperature?

(Multiple Choice)

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Question 58

A concentration-time study of the gas phase reaction 2 A₃ → 3 A₂ produced the data in the table below. Time (s)[A₃] (M)[A₂] (M) 0 4)00 × 10^-4 0 10 2.00 × 10^-4 3.00 × 10^-4 20 1.00 × 10^-4 4.50 × 10^-4 30 5.00 × 10^-5 ? What is the average rate of formation of A₂ in the time interval 20-30 seconds?

(Multiple Choice)

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Question 59

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 12.5% of its initial value?

(Multiple Choice)

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Question 60

Showing 41 - 60 of 206

The half life of the reaction shown below is found not to depend on the concentration of H₂O₂(aq). 2 H₂O₂(aq)→ 2 H₂O(l)+ O₂(g) What is the order of this reaction?

For the reaction shown below,if the rate of formation of Br₂ is 1.2 × 10^-6 M/s,over the same time period the rate of consumption of H⁺ is ________ M/s. ClO₂^-(aq)+ 4 Br^-(aq)+ 4 H⁺(aq)→ Cl^-(aq)+ 2 Br₂(aq)+2 H₂O(l)

Consider a reaction that occurs by the following one-step mechanism: A₂ + B₂ → 2 AB The potential energy profile for this reaction is shown below. -What is the species present at reaction stage 1?

For the reaction shown below,if the rate of formation of O₂ is 6.0 × 10^-6M/s,the rate of decomposition of N₂O₅ over the same time interval is ________. 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)

A reaction has the rate law Rate = k[NO]²[H₂].If the concentration of NO is reduced by 1/3,the rate of reaction will be (increased,decreased)by .

The hydrolysis of tert-butyl chloride is given in the reaction below: (CH₃)₃CCl(aq)+ H₂O(l)→ (CH₃)₃COH(aq)+ H⁺(aq)+ Cl^-(aq) If the rate law is: Rate = k[(CH₃)₃CCl],what is the order of the reaction with respect to water?

The relative initial rates of the reaction A₂ + B₂ → products in vessels (a)-(d)are 1:1:4:4.Unshaded spheres represent A₂ molecules,and shaded spheres represent B₂ molecules present at the beginning of the reaction. -What is the overall order of reaction?

The reaction for the decomposition of dinitrogen monoxide gas to form an oxygen radical is: N₂O(g) $\rarr$ N₂(g)+ O(g).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?

Consider the first-order reaction A → B in which A molecules (unshaded spheres)are converted to B molecules (shaded spheres).Given the following pictures at t = 0 seconds and t = 100 seconds,which picture represents the number of A and B molecules remaining at 200 seconds?

The second-order reaction,2 Mn(CO)₅ → Mn₂(CO)₁₀ has a rate constant equal to 3.0 × 10⁹ M^-1s^-1 at 25°C.If the initial concentration of Mn(CO)₅ is 1.0 × 10^-5 M,how long will it take for 90.% of the reactant to disappear?

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 0.10 M?

The decomposition of cyclopropane,was observed at 500°C and its concentration was monitored as a function of time.The data set is given below.What is the order of the reaction with respect to cyclopropane?

The decay curve shown below approximates the decay of cobalt-60.What is the approximate half-life of cobalt-60?

Acetaldehyde decomposes at 750 K: CH₃CHO → CO + CH₄.The reaction is first order in acetaldehyde and the half-life of the reaction is found to be 530 seconds.What is the rate constant for the reaction at this temperature?

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 12.5% of its initial value?

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Exam 12: Chemical Kinetics

The half life of the reaction shown below is found not to depend on the concentration of H2O2(aq). 2 H2O2(aq)→ 2 H2O(l)+ O2(g) What is the order of this reaction?

The reaction below is second order in ClO2 and first order in OH-.When the concentration of ClO2 is 0.020 M and the concentration of OH- is 0.10 M,the initial rate of reaction is 8.00 × 10-4 M/s.What is the rate constant,k,for this reaction? 2 ClO2(aq)+ 2 OH-(aq)→ ClO3-(aq)+ ClO2-(aq)+ H2O(l)

For the reaction shown below,if the rate of formation of Br2 is 1.2 × 10-6 M/s,over the same time period the rate of consumption of H+ is ________ M/s. ClO2-(aq)+ 4 Br-(aq)+ 4 H+(aq)→ Cl-(aq)+ 2 Br2(aq)+2 H2O(l)

Consider a reaction that occurs by the following one-step mechanism: A2 + B2 → 2 AB The potential energy profile for this reaction is shown below. -What is the species present at reaction stage 1?

For the reaction shown below,if the rate of formation of O2 is 6.0 × 10-6 M/s,the rate of decomposition of N2O5 over the same time interval is ________. 2 N2O5(g)→ 4 NO2(g)+ O2(g)

A reaction has the rate law Rate = k[NO]2[H2].If the concentration of NO is reduced by 1/3,the rate of reaction will be ________ (increased,decreased)by ________.

The hydrolysis of tert-butyl chloride is given in the reaction below: (CH3)3CCl(aq)+ H2O(l)→ (CH3)3COH(aq)+ H+(aq)+ Cl-(aq) If the rate law is: Rate = k[(CH3)3CCl],what is the order of the reaction with respect to water?

The relative initial rates of the reaction A2 + B2 → products in vessels (a)-(d)are 1:1:4:4.Unshaded spheres represent A2 molecules,and shaded spheres represent B2 molecules present at the beginning of the reaction. -What is the overall order of reaction?

The reaction for the decomposition of dinitrogen monoxide gas to form an oxygen radical is: N2O(g) →\rarr→ N2(g)+ O(g).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?

Consider the first-order reaction A → B in which A molecules (unshaded spheres)are converted to B molecules (shaded spheres).Given the following pictures at t = 0 seconds and t = 100 seconds,which picture represents the number of A and B molecules remaining at 200 seconds?

The second-order reaction,2 Mn(CO)5 → Mn2(CO)10 has a rate constant equal to 3.0 × 109 M-1s-1 at 25°C.If the initial concentration of Mn(CO)5 is 1.0 × 10-5 M,how long will it take for 90.% of the reactant to disappear?

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 0.10 M?

The decomposition of cyclopropane,was observed at 500°C and its concentration was monitored as a function of time.The data set is given below.What is the order of the reaction with respect to cyclopropane?

The decay curve shown below approximates the decay of cobalt-60.What is the approximate half-life of cobalt-60?

Acetaldehyde decomposes at 750 K: CH3CHO → CO + CH4.The reaction is first order in acetaldehyde and the half-life of the reaction is found to be 530 seconds.What is the rate constant for the reaction at this temperature?

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 12.5% of its initial value?

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The half life of the reaction shown below is found not to depend on the concentration of H₂O₂(aq). 2 H₂O₂(aq)→ 2 H₂O(l)+ O₂(g) What is the order of this reaction?

For the reaction shown below,if the rate of formation of Br₂ is 1.2 × 10^-6 M/s,over the same time period the rate of consumption of H⁺ is ________ M/s. ClO₂^-(aq)+ 4 Br^-(aq)+ 4 H⁺(aq)→ Cl^-(aq)+ 2 Br₂(aq)+2 H₂O(l)

Consider a reaction that occurs by the following one-step mechanism: A₂ + B₂ → 2 AB The potential energy profile for this reaction is shown below. -What is the species present at reaction stage 1?

For the reaction shown below,if the rate of formation of O₂ is 6.0 × 10^-6M/s,the rate of decomposition of N₂O₅ over the same time interval is ________. 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)

A reaction has the rate law Rate = k[NO]²[H₂].If the concentration of NO is reduced by 1/3,the rate of reaction will be (increased,decreased)by .

The hydrolysis of tert-butyl chloride is given in the reaction below: (CH₃)₃CCl(aq)+ H₂O(l)→ (CH₃)₃COH(aq)+ H⁺(aq)+ Cl^-(aq) If the rate law is: Rate = k[(CH₃)₃CCl],what is the order of the reaction with respect to water?

The relative initial rates of the reaction A₂ + B₂ → products in vessels (a)-(d)are 1:1:4:4.Unshaded spheres represent A₂ molecules,and shaded spheres represent B₂ molecules present at the beginning of the reaction. -What is the overall order of reaction?

The reaction for the decomposition of dinitrogen monoxide gas to form an oxygen radical is: N₂O(g) $\rarr$ N₂(g)+ O(g).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 second-order reaction,2 Mn(CO)₅ → Mn₂(CO)₁₀ has a rate constant equal to 3.0 × 10⁹ M^-1s^-1 at 25°C.If the initial concentration of Mn(CO)₅ is 1.0 × 10^-5 M,how long will it take for 90.% of the reactant to disappear?

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 0.10 M?

Acetaldehyde decomposes at 750 K: CH₃CHO → CO + CH₄.The reaction is first order in acetaldehyde and the half-life of the reaction is found to be 530 seconds.What is the rate constant for the reaction at this temperature?

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 12.5% of its initial value?