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Solved: This reaction is exothermic. If you were a chemist trying to maximize the amount

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 95P Chapter 15

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 95P

This reaction is exothermic.

If you were a chemist trying to maximize the amount of C2H4Cl2 produced, which of the following might you try?

Assume that the reaction mixture reaches equilibrium.

(a) increasing the reaction volume

(b) removing C2H4Cl2 from the reaction mixture as it

forms

(c) lowering the reaction temperature

(d) adding Cl2

Step-by-Step Solution:
Step 1 of 3

Answer :

This reaction is exothermic.

a) increasing the reaction volume

 Increasing volume would increase the amount of reactants and therefore increase product yield due to increasing the number of reactant particles that would be able to react with each other.

b)removing C2H4Cl2 from the reaction mixture as it forms

 Removal would prevent chance of the product being broken back down into the reactants.

c)lowering the reaction temperature

 Lower the reaction if the reaction is exothermic.according to le chatelier's principle.

d) adding Cl2

 Adding Cl2 would have same effect as A, in that would add more reactants so increase reaction rate.

Step 2 of 3

Chapter 15, Problem 95P is Solved
Step 3 of 3

Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

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Solved: This reaction is exothermic. If you were a chemist trying to maximize the amount