Chapter 7.6, Problem 7.5P

Interpretation Introduction

Interpretation:

The equilibrium constant for the given reaction should be identified.

Concept Introduction:

Equilibrium reaction:

A chemical reaction in which neither reactant converted into product nor product formed completely and remains in a reversible phase known as chemical equilibrium reaction.

Or rate of forward reaction is equal to the rate of backward reaction is said be to chemical equilibrium state.

Equilibrium constant:

It denotes the ratio of product and reactants in concentration term that is expressed by K (equilibrium constant).

Consider an equilibrium reaction:

$\text{aA}\text{+}\text{bB}◰\; \hspace{1em}\text{cC}\text{+}\text{dD}$

Here, a, b, c and d are coefficient.

So, the equilibrium expression for above reaction would be.

$\text{K=}\frac{{\text{[C]}}^{\text{c}}{\text{[D]}}^{\text{d}}}{{\text{[A]}}^{\text{a}}{\text{[B]}}^{\text{b}}}$.