Half-life of the first-order reaction has to be calculated if the reactant concentration decreases from 1.02 × 10 − 3 M to 7.4 × 10 − 4 M in 116.7 sec and also the time that is taken for the reactant concentration to decrease from 7.4 × 10 − 4 M to 2.0 × 10 − 4 M has to be calculated.

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Chapter 13, Problem 13.55QE

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Interpretation:

Half-life of the first-order reaction has to be calculated if the reactant concentration decreases from 1.02×10−3 M to 7.4×10−4 M in 116.7 sec and also the time that is taken for the reactant concentration to decrease from 7.4×10−4 M to 2.0×10−4 M has to be calculated.

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First image: Why can't the molecule C be formed in those conditions Second image: Synthesis for lactone C its not an exam

First image: I have to show the mecanism for the reaction on the left, where the alcohol A is added fast in one portion Second image: I have to show the mecanism of the reaction at the bottom. Also I have to show by mecanism why the reaction wouldn't work if the alcohol was primary

First image: I have to explain why the molecule C is never formed in those conditions. Second image: I have to propose a synthesis for the lactone A

Answer 2

Question

Chapter 13, Problem 13.55QE

Interpretation Introduction

Interpretation:

Half-life of the first-order reaction has to be calculated if the reactant concentration decreases from 1.02×10−3 M to 7.4×10−4 M in 116.7 sec and also the time that is taken for the reactant concentration to decrease from 7.4×10−4 M to 2.0×10−4 M has to be calculated.

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Answer 3

Question

Chapter 13, Problem 13.55QE

Interpretation Introduction

Interpretation:

Half-life of the first-order reaction has to be calculated if the reactant concentration decreases from 1.02×10−3 M to 7.4×10−4 M in 116.7 sec and also the time that is taken for the reactant concentration to decrease from 7.4×10−4 M to 2.0×10−4 M has to be calculated.

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Answer 4

Question

Chapter 13, Problem 13.55QE

Interpretation Introduction

Interpretation:

Half-life of the first-order reaction has to be calculated if the reactant concentration decreases from 1.02×10−3 M to 7.4×10−4 M in 116.7 sec and also the time that is taken for the reactant concentration to decrease from 7.4×10−4 M to 2.0×10−4 M has to be calculated.

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Answer 5

Chapter 13, Problem 13.55QE

Interpretation Introduction

Interpretation:

Half-life of the first-order reaction has to be calculated if the reactant concentration decreases from 1.02×10−3 M to 7.4×10−4 M in 116.7 sec and also the time that is taken for the reactant concentration to decrease from 7.4×10−4 M to 2.0×10−4 M has to be calculated.

Answer 6

Chapter 13, Problem 13.55QE

Interpretation Introduction

Interpretation:

Half-life of the first-order reaction has to be calculated if the reactant concentration decreases from 1.02×10−3 M to 7.4×10−4 M in 116.7 sec and also the time that is taken for the reactant concentration to decrease from 7.4×10−4 M to 2.0×10−4 M has to be calculated.

Answer 7

Chapter 13, Problem 13.55QE

Interpretation Introduction

Interpretation:

Half-life of the first-order reaction has to be calculated if the reactant concentration decreases from 1.02×10−3 M to 7.4×10−4 M in 116.7 sec and also the time that is taken for the reactant concentration to decrease from 7.4×10−4 M to 2.0×10−4 M has to be calculated.

Answer 8

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Answer 11

Ch. 13 - Prob. 13.1QE Ch. 13 - Prob. 13.2QE Ch. 13 - What is the difference between the integrated and...Ch. 13 - Prob. 13.4QE Ch. 13 - Explain why half-lives are not normally used to...Ch. 13 - Derive an expression for the half-life of a...Ch. 13 - Prob. 13.7QE Ch. 13 - Prob. 13.8QE Ch. 13 - Prob. 13.9QE Ch. 13 - Prob. 13.10QE

Half-life of the first-order reaction has to be calculated if the reactant concentration decreases from 1.02 × 10 − 3 M to 7.4 × 10 − 4 M in 116.7 sec and also the time that is taken for the reactant concentration to decrease from 7.4 × 10 − 4 M to 2.0 × 10 − 4 M has to be calculated.

Solution Summary: The author calculates the half-life of the first-order reaction if the reactant concentration decreases from 1.02 to 7.4 in 116.7mathrmsec.

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Interpretation:

Half-life of the first-order reaction has to be calculated if the reactant concentration decreases from 1.02×10−3 M to 7.4×10−4 M in 116.7 sec and also the time that is taken for the reactant concentration to decrease from 7.4×10−4 M to 2.0×10−4 M has to be calculated.

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Chapter 13 Solutions

Half-life of the first-order reaction has to be calculated if the reactant concentration decreases from 1.02 × 10 − 3 M to 7.4 × 10 − 4 M in 116.7 sec and also the time that is taken for the reactant concentration to decrease from 7.4 × 10 − 4 M to 2.0 × 10 − 4 M has to be calculated.

Solution Summary: The author calculates the half-life of the first-order reaction if the reactant concentration decreases from 1.02 to 7.4 in 116.7mathrmsec.

Videos

Interpretation: Half-life of the first-order reaction has to be calculated if the reactant concentration decreases from 1.02×10−3 M to 7.4×10−4 M in 116.7 sec and also the time that is taken for the reactant concentration to decrease from 7.4×10−4 M to 2.0×10−4 M has to be calculated.

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Chapter 13 Solutions

Interpretation:

Half-life of the first-order reaction has to be calculated if the reactant concentration decreases from 1.02×10−3 M to 7.4×10−4 M in 116.7 sec and also the time that is taken for the reactant concentration to decrease from 7.4×10−4 M to 2.0×10−4 M has to be calculated.