(a) Interpretation: The given reaction is to be shown as second order using the given data. Concept introduction: The rate law/rate equation for a chemical reaction is an equation that indicates the relationship between reaction rate and concentrations or pressures of the reactants and other constant parameters. For zero-order reactions, the reaction rate is independent of the concentration of a reactant. A first order reaction depends on the concentration of only one reactant. The rate of a second-order reaction may be proportional to one concentration squared.

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Answer 1

Question

Chapter 20, Problem 36E

Interpretation Introduction

(a)

Interpretation:

The given reaction is to be shown as second order using the given data.

Concept introduction:

The rate law/rate equation for a chemical reaction is an equation that indicates the relationship between reaction rate and concentrations or pressures of the reactants and other constant parameters. For zero-order reactions, the reaction rate is independent of the concentration of a reactant. A first order reaction depends on the concentration of only one reactant. The rate of a second-order reaction may be proportional to one concentration squared.

Interpretation Introduction

(b)

Interpretation:

The rate constant of reaction should be determined.

Concept introduction:

For second order reaction:

1[A]t−1[A]0=kt

Where, k is rate constant, t is time, [A]_t is concentration of A at time t and [A]_o is the concentration of A at initial time that is at t = 0.

Interpretation Introduction

(c)

Interpretation:

Time at which [ArSO₂H] is equal to 0.05 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Interpretation Introduction

(d)

Interpretation:

Time at which [ArSO₂H] is equal to 0.025 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Interpretation Introduction

(e)

Interpretation:

Time at which [ArSO₂H] is equal to 0.035 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

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Answer 2

Question

Chapter 20, Problem 36E

Interpretation Introduction

(a)

Interpretation:

The given reaction is to be shown as second order using the given data.

Concept introduction:

The rate law/rate equation for a chemical reaction is an equation that indicates the relationship between reaction rate and concentrations or pressures of the reactants and other constant parameters. For zero-order reactions, the reaction rate is independent of the concentration of a reactant. A first order reaction depends on the concentration of only one reactant. The rate of a second-order reaction may be proportional to one concentration squared.

Interpretation Introduction

(b)

Interpretation:

The rate constant of reaction should be determined.

Concept introduction:

For second order reaction:

1[A]t−1[A]0=kt

Where, k is rate constant, t is time, [A]_t is concentration of A at time t and [A]_o is the concentration of A at initial time that is at t = 0.

Interpretation Introduction

(c)

Interpretation:

Time at which [ArSO₂H] is equal to 0.05 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Interpretation Introduction

(d)

Interpretation:

Time at which [ArSO₂H] is equal to 0.025 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Interpretation Introduction

(e)

Interpretation:

Time at which [ArSO₂H] is equal to 0.035 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Expert Solution & Answer

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Check out a sample textbook solution

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Answer 3

Question

Chapter 20, Problem 36E

Interpretation Introduction

(a)

Interpretation:

The given reaction is to be shown as second order using the given data.

Concept introduction:

The rate law/rate equation for a chemical reaction is an equation that indicates the relationship between reaction rate and concentrations or pressures of the reactants and other constant parameters. For zero-order reactions, the reaction rate is independent of the concentration of a reactant. A first order reaction depends on the concentration of only one reactant. The rate of a second-order reaction may be proportional to one concentration squared.

Interpretation Introduction

(b)

Interpretation:

The rate constant of reaction should be determined.

Concept introduction:

For second order reaction:

1[A]t−1[A]0=kt

Where, k is rate constant, t is time, [A]_t is concentration of A at time t and [A]_o is the concentration of A at initial time that is at t = 0.

Interpretation Introduction

(c)

Interpretation:

Time at which [ArSO₂H] is equal to 0.05 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Interpretation Introduction

(d)

Interpretation:

Time at which [ArSO₂H] is equal to 0.025 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Interpretation Introduction

(e)

Interpretation:

Time at which [ArSO₂H] is equal to 0.035 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Expert Solution & Answer

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Answer 4

Question

Chapter 20, Problem 36E

Interpretation Introduction

(a)

Interpretation:

The given reaction is to be shown as second order using the given data.

Concept introduction:

The rate law/rate equation for a chemical reaction is an equation that indicates the relationship between reaction rate and concentrations or pressures of the reactants and other constant parameters. For zero-order reactions, the reaction rate is independent of the concentration of a reactant. A first order reaction depends on the concentration of only one reactant. The rate of a second-order reaction may be proportional to one concentration squared.

Interpretation Introduction

(b)

Interpretation:

The rate constant of reaction should be determined.

Concept introduction:

For second order reaction:

1[A]t−1[A]0=kt

Where, k is rate constant, t is time, [A]_t is concentration of A at time t and [A]_o is the concentration of A at initial time that is at t = 0.

Interpretation Introduction

(c)

Interpretation:

Time at which [ArSO₂H] is equal to 0.05 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Interpretation Introduction

(d)

Interpretation:

Time at which [ArSO₂H] is equal to 0.025 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Interpretation Introduction

(e)

Interpretation:

Time at which [ArSO₂H] is equal to 0.035 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Expert Solution & Answer

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See solution

Answer 5

Chapter 20, Problem 36E

Interpretation Introduction

(a)

Interpretation:

The given reaction is to be shown as second order using the given data.

Concept introduction:

The rate law/rate equation for a chemical reaction is an equation that indicates the relationship between reaction rate and concentrations or pressures of the reactants and other constant parameters. For zero-order reactions, the reaction rate is independent of the concentration of a reactant. A first order reaction depends on the concentration of only one reactant. The rate of a second-order reaction may be proportional to one concentration squared.

Interpretation Introduction

(b)

Interpretation:

The rate constant of reaction should be determined.

Concept introduction:

For second order reaction:

1[A]t−1[A]0=kt

Where, k is rate constant, t is time, [A]_t is concentration of A at time t and [A]_o is the concentration of A at initial time that is at t = 0.

Interpretation Introduction

(c)

Interpretation:

Time at which [ArSO₂H] is equal to 0.05 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Interpretation Introduction

(d)

Interpretation:

Time at which [ArSO₂H] is equal to 0.025 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Interpretation Introduction

(e)

Interpretation:

Time at which [ArSO₂H] is equal to 0.035 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Answer 6

Chapter 20, Problem 36E

Interpretation Introduction

(a)

Interpretation:

The given reaction is to be shown as second order using the given data.

Concept introduction:

The rate law/rate equation for a chemical reaction is an equation that indicates the relationship between reaction rate and concentrations or pressures of the reactants and other constant parameters. For zero-order reactions, the reaction rate is independent of the concentration of a reactant. A first order reaction depends on the concentration of only one reactant. The rate of a second-order reaction may be proportional to one concentration squared.

Answer 7

Chapter 20, Problem 36E

Interpretation Introduction

(a)

Interpretation:

The given reaction is to be shown as second order using the given data.

Concept introduction:

The rate law/rate equation for a chemical reaction is an equation that indicates the relationship between reaction rate and concentrations or pressures of the reactants and other constant parameters. For zero-order reactions, the reaction rate is independent of the concentration of a reactant. A first order reaction depends on the concentration of only one reactant. The rate of a second-order reaction may be proportional to one concentration squared.

Answer 8

Interpretation Introduction

(b)

Interpretation:

The rate constant of reaction should be determined.

Concept introduction:

For second order reaction:

1[A]t−1[A]0=kt

Where, k is rate constant, t is time, [A]_t is concentration of A at time t and [A]_o is the concentration of A at initial time that is at t = 0.

Answer 9

Interpretation Introduction

(b)

Interpretation:

The rate constant of reaction should be determined.

Concept introduction:

For second order reaction:

1[A]t−1[A]0=kt

Where, k is rate constant, t is time, [A]_t is concentration of A at time t and [A]_o is the concentration of A at initial time that is at t = 0.

Answer 10

Interpretation Introduction

(c)

Interpretation:

Time at which [ArSO₂H] is equal to 0.05 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Answer 11

Interpretation Introduction

(c)

Interpretation:

Time at which [ArSO₂H] is equal to 0.05 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Answer 12

Interpretation Introduction

(d)

Interpretation:

Time at which [ArSO₂H] is equal to 0.025 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Answer 13

Interpretation Introduction

(d)

Interpretation:

Time at which [ArSO₂H] is equal to 0.025 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Answer 14

Interpretation Introduction

(e)

Interpretation:

Time at which [ArSO₂H] is equal to 0.035 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Answer 15

Interpretation Introduction

(e)

Interpretation:

Time at which [ArSO₂H] is equal to 0.035 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Answer 16

Expert Solution & Answer

Answer 17

Expert Solution & Answer

Answer 18

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Answer 19

Ch. 20 - In the reaction 2A+BC+3D , reactant A is found to...Ch. 20 - From Figure 20-2 estimate the rate of reaction at...Ch. 20 - In the reaction A products, [A] is found to be...Ch. 20 - In the reaction A products, at t = 0. [A]= 0.1565...Ch. 20 - In the reaction A products. 4.40 min after the...Ch. 20 - Refer to Experiment 2 of Table 20.3 and to...Ch. 20 - For the reaction A+2BC ,the rate of reaction is...Ch. 20 - If the rate of reaction (20.3) is 5.7104 M s-1 ,...Ch. 20 - In the reaction A(g)B(g)+C(g) , the totalpressure...Ch. 20 - At 65C , the half-life for the first-order...

Solution Summary: The author explains that the rate law/rate equation for a chemical reaction indicates the relationship between reaction rate and concentrations or pressures of the reactants and other constant parameters.

Concept explainers

(b)

Interpretation:

The rate constant of reaction should be determined.

Concept introduction:

For second order reaction:

1[A]t−1[A]0=kt

Where, k is rate constant, t is time, [A]_t is concentration of A at time t and [A]_o is the concentration of A at initial time that is at t = 0.

(c)

Interpretation:

Time at which [ArSO₂H] is equal to 0.05 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

(d)

Interpretation:

Time at which [ArSO₂H] is equal to 0.025 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

(e)

Interpretation:

Time at which [ArSO₂H] is equal to 0.035 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Want to see the full answer?

Chapter 20 Solutions

Solution Summary: The author explains that the rate law/rate equation for a chemical reaction indicates the relationship between reaction rate and concentrations or pressures of the reactants and other constant parameters.

Concept explainers

(b) Interpretation: The rate constant of reaction should be determined. Concept introduction: For second order reaction: 1[A]t−1[A]0=kt Where, k is rate constant, t is time, [A]t is concentration of A at time t and [A]o is the concentration of A at initial time that is at t = 0.

(c) Interpretation: Time at which [ArSO2H] is equal to 0.05 M should be determined. Concept introduction: In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

(d) Interpretation: Time at which [ArSO2H] is equal to 0.025 M should be determined. Concept introduction: In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

(e) Interpretation: Time at which [ArSO2H] is equal to 0.035 M should be determined. Concept introduction: In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

Want to see the full answer?

Chapter 20 Solutions

(b)

Interpretation:

The rate constant of reaction should be determined.

Concept introduction:

For second order reaction:

1[A]t−1[A]0=kt

Where, k is rate constant, t is time, [A]_t is concentration of A at time t and [A]_o is the concentration of A at initial time that is at t = 0.

(c)

Interpretation:

Time at which [ArSO₂H] is equal to 0.05 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

(d)

Interpretation:

Time at which [ArSO₂H] is equal to 0.025 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.

(e)

Interpretation:

Time at which [ArSO₂H] is equal to 0.035 M should be determined.

Concept introduction:

In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.