Chapter 15, Problem 47E

Interpretation Introduction

Interpretation:

The given expression is to be checked whether is correctly written or not. If not, write the given expression correctly.

Concept introduction:

For a reaction, equilibrium constant is given by the law of mass action. It is defined as the ratio of concentrations of products to that of reactants each raised to the power of their stoichiometric coefficients. Consider the chemical reaction as follows: $\text{aA}+\text{bB}\rightleftharpoons \text{cC}+\text{dD}$.

The expression for the equilibrium constant 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, $\left[\text{A}\right]$ and $\left[\text{B}\right]$ are the concentrations of the reactants $\text{A}$ and $\text{B}$, $\left[\text{C}\right]$ and $\left[\text{D}\right]$ are the concentrations of the products $\text{C and D}$, and $a,b,c,andd$ are the stoichiometric coefficients. The coefficients given in the chemical equation are represented as exponent in the expression of equilibrium constant.

In a chemical reaction, the concentration of pure liquid or pure solid represented as $\left(l\right)$ and $\left(s\right)$ does not change. Hence, these concentrations of reactant or product given as solids and liquids are not expressed in the expression of equilibrium constant.