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 mol L-1 to 3.50 × 10-2 mol L-1. What is the rate constant for the reaction at this temperature?

A) 5.12 × 10-4 L mol-1 s-1 B) 9.69 × 10-2 L mol-1 s-1 C) 10.3 L mol-1 s-1 D) 1.95 × 103 L mol-1 s-1 A) 5.12 × 10-4 L mol-1 s-1 B) 9.69 × 10-2 L mol-1 s-1 C) 10.3 L mol-1 s-1 D) 1.95 × 103 L mol-1 s-1

Calculate the activation energy, Ea, for a reaction with a frequency factor, A, of 9.3 × 1010 s-1 and a rate constant of 1.06 × 103 s-1 at 273 K.

A) 42 kJ mol-1 B) 45 kJ mol-1 C) 36 kJ mol-1 D) 49 kJ mol-1 E) 58 kJ mol-1 A) 42 kJ mol-1 B) 45 kJ mol-1 C) 36 kJ mol-1 D) 49 kJ mol-1 E) 58 kJ mol-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.

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N2O5(g)→ 4NO2(g)+ O2(g). If the rate of disappearance of N2O5 is equal to 1.60 mol min-1 at a particular moment, what is the rate of appearance of NO2 at that moment?

A) 0.800 mol min-1 B) 1.60 mol min-1 C) 3.20 mol min-1 D) 6.40 mol min-1 A) 0.800 mol min-1 B) 1.60 mol min-1 C) 3.20 mol min-1 D) 6.40 mol min-1

The second-order decomposition of NO2 has a rate constant of 0.255 L mol-1 s-1. How much NO2 decomposes in 4.00 s if the initial concentration of NO2 (1.00 L volume)is 1.33 mol L-1?

A) 1.8 mol B) 0.85 mol C) 0.48 mol D) 0.77 mol E) 0.56 mol A) 1.8 mol B) 0.85 mol C) 0.48 mol D) 0.77 mol E) 0.56 mol

Exam 13: Chemical Kinetics

The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10^-4 s^-1. If the initial concentration of cyclopropane is 1.33 mol L^-1, what is the concentration of cyclopropane after 644 s?

(Multiple Choice)

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Question 121

Calculate the frequency factor, A, for a reaction with a rate constant of 7834 s^-1 and an activation energy, E_a, of 68.4 kJ mol^-1 at 305 K.

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Question 122

If a reaction carried out at 61 ◦C has an activation energy, E_a, of 67.3 kJ mol^-1, a rate constant of 791 s^-1, and a frequency factor, A, of 2.65 × 10¹³, what is the value of R? k = A

(Multiple Choice)

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Question 123

Match the following. -t_1/2

(Multiple Choice)

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Question 124

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value?

(Multiple Choice)

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Question 125

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 mol L^-1 to 3.50 × 10^-2 mol L^-1. What is the rate constant for the reaction at this temperature?

(Multiple Choice)

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Question 126

Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X][Y]²

(Multiple Choice)

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Question 127

Calculate the activation energy, E_a, for a reaction with a frequency factor, A, of 9.3 × 10¹⁰ s^-1 and a rate constant of 1.06 × 10³ s^-1 at 273 K.

(Multiple Choice)

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Question 128

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 129

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N₂O₅(g)→ 4NO₂(g)+ O₂(g). If the rate of disappearance of N₂O₅ is equal to 1.60 mol min^-1 at a particular moment, what is the rate of appearance of NO₂ at that moment?

(Multiple Choice)

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Question 130

Given the following balanced equation, determine the rate of reaction with respect to [O₂]. 2SO₂(g)+ O₂(g)→ 2SO₃(g)

(Multiple Choice)

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Question 131

Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration:

(Multiple Choice)

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Question 132

What is the activation energy for a reaction that has a rate constant of 5.68 × 10^-8 s^-1at 298 K and 1.73 × 10^-5 s^-1 at 348 K?

(Multiple Choice)

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Question 133

Which of the following represents the equation for a first-order half-life?

(Multiple Choice)

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Question 134

What is the difference between average reaction rate and instantaneous reaction rate?

(Essay)

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Question 135

What are the units of k in the following rate law? Rate = k[X]²

(Multiple Choice)

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Question 136

The second-order decomposition of NO₂ has a rate constant of 0.255 L mol^-1s^-1. How much NO₂ decomposes in 4.00 s if the initial concentration of NO₂ (1.00 L volume)is 1.33 mol L^-1?

(Multiple Choice)

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Question 137

What are the units of k in a zero-order reaction?

(Multiple Choice)

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Question 138

A reaction is found to have an activation energy of 38.0 kJ mol^-1. If the rate constant for this reaction is 1.60 × 10² L mol^-1s^-1 at 249 K, what is the rate constant at 436 K?

(Multiple Choice)

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Question 139

Is the activation energy for a forward reaction the same as the activation energy for the reverse of the same reaction? Use a sketch of a reaction energy diagram.

(Essay)

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Question 140

Showing 121 - 140 of 162

Exam 13: Chemical Kinetics

The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10-4 s-1. If the initial concentration of cyclopropane is 1.33 mol L-1, what is the concentration of cyclopropane after 644 s?

Calculate the frequency factor, A, for a reaction with a rate constant of 7834 s-1 and an activation energy, Ea, of 68.4 kJ mol-1 at 305 K.

If a reaction carried out at 61 ◦C has an activation energy, Ea, of 67.3 kJ mol-1, a rate constant of 791 s-1, and a frequency factor, A, of 2.65 × 1013, what is the value of R? k = A

Match the following. -t1/2

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value?

Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X][Y]2

Calculate the activation energy, Ea, for a reaction with a frequency factor, A, of 9.3 × 1010 s-1 and a rate constant of 1.06 × 103 s-1 at 273 K.

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?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N2O5(g)→ 4NO2(g)+ O2(g). If the rate of disappearance of N2O5 is equal to 1.60 mol min-1 at a particular moment, what is the rate of appearance of NO2 at that moment?

Given the following balanced equation, determine the rate of reaction with respect to [O2]. 2SO2(g)+ O2(g)→ 2SO3(g)

Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration:

What is the activation energy for a reaction that has a rate constant of 5.68 × 10-8 s-1 at 298 K and 1.73 × 10-5 s-1 at 348 K?

Which of the following represents the equation for a first-order half-life?

What is the difference between average reaction rate and instantaneous reaction rate?

What are the units of k in the following rate law? Rate = k[X]2

The second-order decomposition of NO2 has a rate constant of 0.255 L mol-1 s-1. How much NO2 decomposes in 4.00 s if the initial concentration of NO2 (1.00 L volume)is 1.33 mol L-1?

What are the units of k in a zero-order reaction?

A reaction is found to have an activation energy of 38.0 kJ mol-1. If the rate constant for this reaction is 1.60 × 102 L mol-1 s-1 at 249 K, what is the rate constant at 436 K?

Is the activation energy for a forward reaction the same as the activation energy for the reverse of the same reaction? Use a sketch of a reaction energy diagram.

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The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10^-4 s^-1. If the initial concentration of cyclopropane is 1.33 mol L^-1, what is the concentration of cyclopropane after 644 s?

Calculate the frequency factor, A, for a reaction with a rate constant of 7834 s^-1 and an activation energy, E_a, of 68.4 kJ mol^-1 at 305 K.

If a reaction carried out at 61 ◦C has an activation energy, E_a, of 67.3 kJ mol^-1, a rate constant of 791 s^-1, and a frequency factor, A, of 2.65 × 10¹³, what is the value of R? k = A

Match the following. -t_1/2

Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X][Y]²

Calculate the activation energy, E_a, for a reaction with a frequency factor, A, of 9.3 × 10¹⁰ s^-1 and a rate constant of 1.06 × 10³ s^-1 at 273 K.

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?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N₂O₅(g)→ 4NO₂(g)+ O₂(g). If the rate of disappearance of N₂O₅ is equal to 1.60 mol min^-1 at a particular moment, what is the rate of appearance of NO₂ at that moment?

Given the following balanced equation, determine the rate of reaction with respect to [O₂]. 2SO₂(g)+ O₂(g)→ 2SO₃(g)

What is the activation energy for a reaction that has a rate constant of 5.68 × 10^-8 s^-1at 298 K and 1.73 × 10^-5 s^-1 at 348 K?

What are the units of k in the following rate law? Rate = k[X]²

The second-order decomposition of NO₂ has a rate constant of 0.255 L mol^-1s^-1. How much NO₂ decomposes in 4.00 s if the initial concentration of NO₂ (1.00 L volume)is 1.33 mol L^-1?

A reaction is found to have an activation energy of 38.0 kJ mol^-1. If the rate constant for this reaction is 1.60 × 10² L mol^-1s^-1 at 249 K, what is the rate constant at 436 K?