Chapter 15, Problem 55E

Interpretation Introduction

Interpretation:

For the given concentrations of products, the equilibrium constant $\left(K_{\text{eq}}\right)$ value should be calculated.

Concept Introduction:

Equilibrium may be defined as a state at which the rate of forward reaction is equal to the rate of backward reaction.

The equilibrium constant is the ratio of concentrations of products to that of reactants each raised to the power of their stoichiometric coefficients. Consider the general chemical reaction as follows: $\text{aA}+\text{bB}\rightleftharpoons \text{cC}+\text{dD}$.

The equilibrium constant expression for the above reaction is written as

$K_{\text{eq}}=\frac{{\left[\text{C}\right]}^c{\left[\text{D}\right]}^d}{{\left[\text{A}\right]}^a{\left[\text{B}\right]}^b}$

Here, the reactants are $\text{A}$ and $\text{B}$, the products are $\text{C and D}$, and the stoichiometric coefficients are $a,b,c,andd$.