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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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Given the reaction A + B C + D , consider the following situations:
a. You have 1.3 M A and 0.8 M B initially.
b. You have 1.3 M A, 0.8 M B, and 0.2 M C initially.
c. You have 2.0 M A and 0.8 M B initially.
Order the preceding situations in terms of increasing equilibrium concentration of D and explain your order. Give the order in terms of increasing equilibrium concentration of B and explain.

Interpretation Introduction

Interpretation:

The order of the given situations in the terms of increasing equilibrium concentration of D is to be stated and the order in terms of increasing equilibrium concentration of B is to be stated with an explanation.

Concept Introduction:

In a chemical equilibrium the concentration of the reactants and products remain constant. The rate of the forward reaction is equal to the rate of backward reaction. According to the Le Chatelier’s Principle, the equilibrium shifts in such a way or a direction that the effect of change is reduced.

Explanation

The given reaction is A+ C+D and the situations are as follows:

  • The initial concentration of A and B is 1.3 M and 0.8 M.
  • The initial concentration of A, B and C is 1.3 M, 0.8 M and 0.2 M.
  • The initial concentration of A and B is 2.0 M and 0.8 M.

It is assumed that the situation a is the reference point and product C and D are not formed.

In situation b, the initial concentration of A, B and C is 1.3 M, 0.8 M and 0.2 M.The concentration of A and B is same to the reference point but it is assumed that the product C is not formed in the reference point. The concentration of C shifts the equilibrium towards the left side or in backward direction which results in the decrease in the concentration of D

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