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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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Although the equilibrium constant for a given reaction always has the same value at the same temperature, the actual concentrations present at equilibrium may differ from one experiment to another. Explain. What do we mean by an equilibrium position? Is the equilibrium position always the same for a reaction, regardless of the amounts of reactants taken?

Interpretation Introduction

Interpretation:

An explanation for the same value of equilibrium constant at the same temperature for a given reaction, but difference in the actual concentrations at equilibrium from one experiment to another is to be stated. The meaning of an equilibrium position is to be stated. Whether the equilibrium position always the same for a reaction, regardless of the amounts of reactants taken or not is to be predicted.

Concept Introduction:

The chemical equilibrium is the state in which the rates of both forward and backward reactions become equal. The concentration of both reactants and products do not change on reaching an equilibrium state.

The general chemical equation is shown below.

aA+bBcC+dD

The general equilibrium expression for a reaction is shown below.

K=[C]c[D]d[A]a[B]b

Where,

  • K is an equilibrium constant.

In the above expression, square brackets represent the concentrations of both reactants and products.

Explanation

The equilibrium expression for a reactions exhibits that equilibrium constant is the ratio of concentrations of products raised to the power of their coefficients and concentrations of reactants raised to the power of their coefficients. Thus, the value of the equilibrium constant does not change. However, the concentrations at equilibrium in different situations can be different...

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