Consider the reaction NOBr(g)$\rightarrow$ NO(g)+ ½Br2(g) A plot of [NOBr]-sup>1 vs t gives a straight line with a slope of 2.00 M-1.s-1.The order of the reaction and the rate constant,Respectively,Are

A) second-order and 0.500 M-1.s-1. B) first-order and 2.00 s-1. C) second-order and 2.00 M-1.s-1 D) first-order and 0.241 s-1. E) second-order and 16.6 M-1.s-1 A) second-order and 0.500 M-1.s-1. B) first-order and 2.00 s-1. C) second-order and 2.00 M-1.s-1 D) first-order and 0.241 s-1. E) second-order and 16.6 M-1.s-1

A first-order reaction has a rate constant of 0.00300 s-1 .The time required for 60% reaction is

A) 153 s. B) 73.9 s. C) 170 s. D) 133 s. E) 305 s. A) 153 s. B) 73.9 s. C) 170 s. D) 133 s. E) 305 s.

If the average rate of formation of H2(g) is 3.90 (mol H2).L-1.s-1 for the reaction2PH3(g)$\rightarrow$2P(g)+ 3H2(g),The unique average reaction rate is

A) 3.90 mol.L-1.s-1. B) 1.30 mol.L-1.s-1. C) 2.60 mol.L-1.s-1. D) 7.80 mol.L-1.s-1. E) 11.7 mol.L-1.s-1. A) 3.90 mol.L-1.s-1. B) 1.30 mol.L-1.s-1. C) 2.60 mol.L-1.s-1. D) 7.80 mol.L-1.s-1. E) 11.7 mol.L-1.s-1.

Consider the reaction 2N2O5(g)$\rightarrow$ 4NO2(g)+ O2(g) Rate = k[N2O5] Calculate the time for the concentration of N2O5 to fall to one-fourth its initial value if the half-life is 133 s.

A) 133 s B) 33.3 s C) 266 s D) 66.6 s E) 533 s A) 133 s B) 33.3 s C) 266 s D) 66.6 s E) 533 s

If the average rate of decomposition of PH3(g) is 3.2 (mol PH3).L-1.min-1 for the reaction 2PH3(g)$\rightarrow$ 2P(g)+ 3H2(g), The unique average reaction rate is

A) 3.2 mol.L-1.min-1. B) 2.1 mol.L-1.min-1. C) 1.6 mol.L-1.min-1. D) 4.8 mol.L-1.min-1. E) 6.4 mol.L-1.min-1. A) 3.2 mol.L-1.min-1. B) 2.1 mol.L-1.min-1. C) 1.6 mol.L-1.min-1. D) 4.8 mol.L-1.min-1. E) 6.4 mol.L-1.min-1.

Consider the following mechanism for the destruction of ozone. O3 + NO $\rarr$ NO2 + O2 NO2 + O$\rarr$ NO + O2 What is the catalyst in this reaction?

The answer of Consider the following mechanism for the destruction...

Consider the reaction 2N2O(g)$\rightarrow$2N2(g)+ O2(g) Rate = k[N2O]For an initial concentration of N2O of 0.50 M,What is the concentration of N2O remaining after 2.0 min if k = 3.4 * 10-3 s-1?

A) 0.50 M B) 0.55 M C) 0.66 M D) 0.33 M E) 0.17 M A) 0.50 M B) 0.55 M C) 0.66 M D) 0.33 M E) 0.17 M

A second-order reaction has a rate constant of 1.25 M-1.s-1 .If the initial reactant concentration is 1.0 M,Calculate the time required for 90% reaction.

A) 1.3 s B) 7.2 s C) 0.13 s D) 17 s E) 0.89 s A) 1.3 s B) 7.2 s C) 0.13 s D) 17 s E) 0.89 s

The reaction profile for the mechanism NO2(g)+ F2(g)$\rightarrow$NO2F(g)+ F(g) Slow F(g)+ NO2(g)$\rightarrow$NO2F(g) Fast Shows

A) two maxima, the first maximum being the higher. B) two maxima, the second maximum being the higher. C) one maximum for the second step. D) two maxima, both the same height. A) two maxima, the first maximum being the higher. B) two maxima, the second maximum being the higher. C) one maximum for the second step. D) two maxima, both the same height.

The reduction of M3+ by Cr2+ was studied with [Cr2+] 100 times the concentration of Cr2+ .When [Cr2+] = 0.0050 M,The rate was 2.5 s-1.The rate constant for this reaction is

A) 1.3 M-1·s-1 B) 0.013 M-1·s-1 C) 5.0 M-1·s-1 D) 500 M-1·s-1 A) 1.3 M-1·s-1 B) 0.013 M-1·s-1 C) 5.0 M-1·s-1 D) 500 M-1·s-1

Exam 7: Kinetics

Consider the reaction NOBr(g) $\rightarrow$ NO(g)+ ½Br₂(g) A plot of [NOBr]^-sup>1 vs t gives a straight line with a slope of 2.00 M^-¹.s^-¹.The order of the reaction and the rate constant,Respectively,Are

(Multiple Choice)

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Question 61

A first-order reaction has a rate constant of 0.00300 s^-¹ .The time required for 60% reaction is

(Multiple Choice)

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Question 62

If the average rate of formation of H₂(g) is 3.90 (mol H₂).L^-¹.s^-¹ for the reaction2PH₃(g) $\rightarrow$ 2P(g)+ 3H₂(g),The unique average reaction rate is

(Multiple Choice)

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Question 63

For a second-order reaction, a straight line is obtained from a plot of

(Multiple Choice)

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Question 64

Consider the reaction 2N₂O₅(g) $\rightarrow$ 4NO₂(g)+ O₂(g) Rate = k[N₂O₅] Calculate the time for the concentration of N₂O₅ to fall to one-fourth its initial value if the half-life is 133 s.

(Multiple Choice)

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Question 65

What is the rate constant for a first-order reaction with a half-life of 9.0 ms?

(Multiple Choice)

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Question 66

If the average rate of decomposition of PH₃(g) is 3.2 (mol PH₃).L^-¹.min^-¹ for the reaction 2PH₃(g) $\rightarrow$ 2P(g)+ 3H₂(g), The unique average reaction rate is

(Multiple Choice)

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Question 67

An elementary process has an activation energy of 92 kJ/mol .If the enthalpy change for the reaction is -62 kJ/mol, What is the activation energy for the reverse reaction?

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Question 68

Consider the mechanism ClO^-(aq)+ H₂O(l) $f$ HOCl(aq)+ OH^-(aq) K,fast I^-(aq)+ HOCl(aq) $\rightarrow$ HOI(aq)+ Cl^-(aq) k,slow HOI(aq)+ OH^-(aq) $\rightarrow$ OI^-(aq)+ H₂O(l) k,fast Draw the reaction profile for this mechanism.

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Question 69

Consider the following mechanism for the destruction of ozone. O₃ + NO $\rarr$ NO₂ + O₂ NO₂ + O $\rarr$ NO + O₂ What is the catalyst in this reaction?

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Question 70

Consider the reaction 2N₂O(g) $\rightarrow$ 2N₂(g)+ O₂(g) Rate = k[N₂O]For an initial concentration of N₂O of 0.50 M,What is the concentration of N₂O remaining after 2.0 min if k = 3.4 * 10^-³ s^-¹?

(Multiple Choice)

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Question 71

A second-order reaction has a rate constant of 1.25 M^-¹.s^-¹ .If the initial reactant concentration is 1.0 M,Calculate the time required for 90% reaction.

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Question 72

The concentration-time dependence is shown below for two first-order reactions is: Which reaction has the larger rate constant?

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Question 73

A catalyst facilitates a reaction by

(Multiple Choice)

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Question 74

What is the half-life of a reaction that has a rate constant of 280 s^-¹?

(Multiple Choice)

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Question 75

The reaction profile for the mechanism NO₂(g)+ F₂(g) $\rightarrow$ NO₂F(g)+ F(g) Slow F(g)+ NO₂(g) $\rightarrow$ NO₂F(g) Fast Shows

(Multiple Choice)

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Question 76

The reduction of M³⁺ by Cr²⁺ was studied with [Cr²⁺] 100 times the concentration of Cr²⁺ .When [Cr²⁺] = 0.0050 M,The rate was 2.5 s^-¹.The rate constant for this reaction is

(Multiple Choice)

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Question 77

If the rate of a reaction increases by a factor of 64 when the concentration of reactant increases by a factor of 4, the order of the reaction with respect to this reactant is

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Question 78

The rate law for the following mechanism is ClO^-(aq)+ H₂O(l) $f$ HOCl(aq)+ OH^-(aq) K,Fast I^-(aq)+ HOCl(aq) $\rightarrow$ HOI(aq)+ Cl^-(aq) K₁,Slow HOI(aq)+ OH^-(aq) $\rightarrow$ OI^-(aq)+ H₂O(l) K₂,Fast

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Question 79

Technetium-99m, used to image the heart and brain,Has a half-life of 6.00 h. What fraction of technetium-99m remains in the body after 1 day?

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Question 80

Showing 61 - 80 of 87

Consider the reaction NOBr(g) $\rightarrow$ NO(g)+ ½Br₂(g) A plot of [NOBr]^-sup>1 vs t gives a straight line with a slope of 2.00 M^-¹.s^-¹.The order of the reaction and the rate constant,Respectively,Are

A first-order reaction has a rate constant of 0.00300 s^-¹ .The time required for 60% reaction is

If the average rate of formation of H₂(g) is 3.90 (mol H₂).L^-¹.s^-¹ for the reaction2PH₃(g) $\rightarrow$ 2P(g)+ 3H₂(g),The unique average reaction rate is

For a second-order reaction, a straight line is obtained from a plot of

Consider the reaction 2N₂O₅(g) $\rightarrow$ 4NO₂(g)+ O₂(g) Rate = k[N₂O₅] Calculate the time for the concentration of N₂O₅ to fall to one-fourth its initial value if the half-life is 133 s.

What is the rate constant for a first-order reaction with a half-life of 9.0 ms?

If the average rate of decomposition of PH₃(g) is 3.2 (mol PH₃).L^-¹.min^-¹ for the reaction 2PH₃(g) $\rightarrow$ 2P(g)+ 3H₂(g), The unique average reaction rate is

An elementary process has an activation energy of 92 kJ/mol .If the enthalpy change for the reaction is -62 kJ/mol, What is the activation energy for the reverse reaction?

Consider the mechanism ClO^-(aq)+ H₂O(l) $f$ HOCl(aq)+ OH^-(aq) K,fast I^-(aq)+ HOCl(aq) $\rightarrow$ HOI(aq)+ Cl^-(aq) k,slow HOI(aq)+ OH^-(aq) $\rightarrow$ OI^-(aq)+ H₂O(l) k,fast Draw the reaction profile for this mechanism.

Consider the following mechanism for the destruction of ozone. O₃ + NO $\rarr$ NO₂ + O₂ NO₂ + O $\rarr$ NO + O₂ What is the catalyst in this reaction?

Consider the reaction 2N₂O(g) $\rightarrow$ 2N₂(g)+ O₂(g) Rate = k[N₂O]For an initial concentration of N₂O of 0.50 M,What is the concentration of N₂O remaining after 2.0 min if k = 3.4 * 10^-³ s^-¹?

A second-order reaction has a rate constant of 1.25 M^-¹.s^-¹ .If the initial reactant concentration is 1.0 M,Calculate the time required for 90% reaction.

The concentration-time dependence is shown below for two first-order reactions is: Which reaction has the larger rate constant?

A catalyst facilitates a reaction by

What is the half-life of a reaction that has a rate constant of 280 s^-¹?

The reaction profile for the mechanism NO₂(g)+ F₂(g) $\rightarrow$ NO₂F(g)+ F(g) Slow F(g)+ NO₂(g) $\rightarrow$ NO₂F(g) Fast Shows

The reduction of M³⁺ by Cr²⁺ was studied with [Cr²⁺] 100 times the concentration of Cr²⁺ .When [Cr²⁺] = 0.0050 M,The rate was 2.5 s^-¹.The rate constant for this reaction is

If the rate of a reaction increases by a factor of 64 when the concentration of reactant increases by a factor of 4, the order of the reaction with respect to this reactant is

The rate law for the following mechanism is ClO^-(aq)+ H₂O(l) $f$ HOCl(aq)+ OH^-(aq) K,Fast I^-(aq)+ HOCl(aq) $\rightarrow$ HOI(aq)+ Cl^-(aq) K₁,Slow HOI(aq)+ OH^-(aq) $\rightarrow$ OI^-(aq)+ H₂O(l) K₂,Fast

Technetium-99m, used to image the heart and brain,Has a half-life of 6.00 h. What fraction of technetium-99m remains in the body after 1 day?

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Exam 7: Kinetics

Consider the reaction NOBr(g) →\rightarrow→ NO(g)+ ½Br2(g) A plot of [NOBr]-sup>1 vs t gives a straight line with a slope of 2.00 M-1.s-1.The order of the reaction and the rate constant,Respectively,Are

A first-order reaction has a rate constant of 0.00300 s-1 .The time required for 60% reaction is

If the average rate of formation of H2(g) is 3.90 (mol H2).L-1.s-1 for the reaction2PH3(g) →\rightarrow→ 2P(g)+ 3H2(g),The unique average reaction rate is

For a second-order reaction, a straight line is obtained from a plot of

Consider the reaction 2N2O5(g) →\rightarrow→ 4NO2(g)+ O2(g) Rate = k[N2O5] Calculate the time for the concentration of N2O5 to fall to one-fourth its initial value if the half-life is 133 s.

What is the rate constant for a first-order reaction with a half-life of 9.0 ms?

If the average rate of decomposition of PH3(g) is 3.2 (mol PH3).L-1.min-1 for the reaction 2PH3(g) →\rightarrow→ 2P(g)+ 3H2(g), The unique average reaction rate is

An elementary process has an activation energy of 92 kJ/mol .If the enthalpy change for the reaction is -62 kJ/mol, What is the activation energy for the reverse reaction?

Consider the mechanism ClO-(aq)+ H2O(l) fff HOCl(aq)+ OH-(aq) K,fast I-(aq)+ HOCl(aq) →\rightarrow→ HOI(aq)+ Cl-(aq) k,slow HOI(aq)+ OH-(aq) →\rightarrow→ OI-(aq)+ H2O(l) k,fast Draw the reaction profile for this mechanism.

Consider the following mechanism for the destruction of ozone. O3 + NO →\rarr→ NO2 + O2 NO2 + O →\rarr→ NO + O2 What is the catalyst in this reaction?

Consider the reaction 2N2O(g) →\rightarrow→ 2N2(g)+ O2(g) Rate = k[N2O]For an initial concentration of N2O of 0.50 M,What is the concentration of N2O remaining after 2.0 min if k = 3.4 * 10-3 s-1?

A second-order reaction has a rate constant of 1.25 M-1.s-1 .If the initial reactant concentration is 1.0 M,Calculate the time required for 90% reaction.

The concentration-time dependence is shown below for two first-order reactions is: Which reaction has the larger rate constant?

A catalyst facilitates a reaction by

What is the half-life of a reaction that has a rate constant of 280 s-1?

The reaction profile for the mechanism NO2(g)+ F2(g) →\rightarrow→ NO2F(g)+ F(g) Slow F(g)+ NO2(g) →\rightarrow→ NO2F(g) Fast Shows

The reduction of M3+ by Cr2+ was studied with [Cr2+] 100 times the concentration of Cr2+ .When [Cr2+] = 0.0050 M,The rate was 2.5 s-1.The rate constant for this reaction is

If the rate of a reaction increases by a factor of 64 when the concentration of reactant increases by a factor of 4, the order of the reaction with respect to this reactant is

The rate law for the following mechanism is ClO-(aq)+ H2O(l) fff HOCl(aq)+ OH-(aq) K,Fast I-(aq)+ HOCl(aq) →\rightarrow→ HOI(aq)+ Cl-(aq) K1,Slow HOI(aq)+ OH-(aq) →\rightarrow→ OI-(aq)+ H2O(l) K2,Fast

Technetium-99m, used to image the heart and brain,Has a half-life of 6.00 h. What fraction of technetium-99m remains in the body after 1 day?

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Reactions

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

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Consider the reaction NOBr(g) $\rightarrow$ NO(g)+ ½Br₂(g) A plot of [NOBr]^-sup>1 vs t gives a straight line with a slope of 2.00 M^-¹.s^-¹.The order of the reaction and the rate constant,Respectively,Are

A first-order reaction has a rate constant of 0.00300 s^-¹ .The time required for 60% reaction is

If the average rate of formation of H₂(g) is 3.90 (mol H₂).L^-¹.s^-¹ for the reaction2PH₃(g) $\rightarrow$ 2P(g)+ 3H₂(g),The unique average reaction rate is

Consider the reaction 2N₂O₅(g) $\rightarrow$ 4NO₂(g)+ O₂(g) Rate = k[N₂O₅] Calculate the time for the concentration of N₂O₅ to fall to one-fourth its initial value if the half-life is 133 s.

If the average rate of decomposition of PH₃(g) is 3.2 (mol PH₃).L^-¹.min^-¹ for the reaction 2PH₃(g) $\rightarrow$ 2P(g)+ 3H₂(g), The unique average reaction rate is

Consider the mechanism ClO^-(aq)+ H₂O(l) $f$ HOCl(aq)+ OH^-(aq) K,fast I^-(aq)+ HOCl(aq) $\rightarrow$ HOI(aq)+ Cl^-(aq) k,slow HOI(aq)+ OH^-(aq) $\rightarrow$ OI^-(aq)+ H₂O(l) k,fast Draw the reaction profile for this mechanism.

Consider the following mechanism for the destruction of ozone. O₃ + NO $\rarr$ NO₂ + O₂ NO₂ + O $\rarr$ NO + O₂ What is the catalyst in this reaction?

Consider the reaction 2N₂O(g) $\rightarrow$ 2N₂(g)+ O₂(g) Rate = k[N₂O]For an initial concentration of N₂O of 0.50 M,What is the concentration of N₂O remaining after 2.0 min if k = 3.4 * 10^-³ s^-¹?

A second-order reaction has a rate constant of 1.25 M^-¹.s^-¹ .If the initial reactant concentration is 1.0 M,Calculate the time required for 90% reaction.

What is the half-life of a reaction that has a rate constant of 280 s^-¹?

The reaction profile for the mechanism NO₂(g)+ F₂(g) $\rightarrow$ NO₂F(g)+ F(g) Slow F(g)+ NO₂(g) $\rightarrow$ NO₂F(g) Fast Shows

The reduction of M³⁺ by Cr²⁺ was studied with [Cr²⁺] 100 times the concentration of Cr²⁺ .When [Cr²⁺] = 0.0050 M,The rate was 2.5 s^-¹.The rate constant for this reaction is

The rate law for the following mechanism is ClO^-(aq)+ H₂O(l) $f$ HOCl(aq)+ OH^-(aq) K,Fast I^-(aq)+ HOCl(aq) $\rightarrow$ HOI(aq)+ Cl^-(aq) K₁,Slow HOI(aq)+ OH^-(aq) $\rightarrow$ OI^-(aq)+ H₂O(l) K₂,Fast