Chapter 15.5, Problem 15.5.2SR

Interpretation Introduction

Interpretation:

Using given equilibrium constant value, the concentration of A, B and C in given equilibrium reaction has to be calculated.

Concept Information:

Equilibrium expression: The equilibrium expression is equal to the concentration of each product raised to its coefficient in a balanced chemical equation and multiplied together, divides by the concentrate ions of the product of reactants to the power of their coefficient.

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one, the reaction will move to the right side of reaction.

Homogeneous equilibrium: A homogeneous equilibrium involved has a everything present in the same phase and same conditions, for example reactions where everything is a gas, or everything is present in the same solution.

Heterogeneous equilibrium: This equilibrium reaction does not depend on the amounts of pure solid and liquid present, in other words heterogeneous equilibrium, substances are in different phases.

Equilibrium constant (${\text{K}}_{\text{c}}$ ):

In the equilibrium reaction, the ratio of concentration of the reactant and concentration of the product.

Reaction quotient (Q): It is defined as the ratio between concentration of the product and concentration of the reactant.

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

This value used to know about the direction of the reaction is going to proceed.

If $\text{Q = K}$ means the reaction reached the equilibrium.

If $\text{Q > K}$ means, the reaction must go to left.

If $\text{Q < K}$ means, the reaction must go to right.