Chapter 15, Problem 14E

Interpretation Introduction

Interpretation: Consider the following condition and find out the direction of the reaction

(1) Q < K

(2) Q > K

(3) Q = K

Concept introduction: Equilibrium is the condition at which the concentration of the reactant and the product are equal and the reaction can in move either forward means towards product formation or backward reaction means towards reactant formation.

Equilibrium constant K_c is defined as the ratio of the concentrations of the products raised to the power of their stoichiometric coefficients and reactants raised to the power of their stoichiometric coefficients.

Reaction quotient Q is defined as the ratio at any point of the reaction of the concentration of the product raised to the power of their stoichiometric coefficients and reactant raised to the power of their stoichiometric coefficients.

aA + bB→cC + dD

$K_c=\frac{{\left[C\right]}^c{\left[D\right]}^d}{{\left[A\right]}^a{\left[B\right]}^b}$, equilibrium

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

To find: The direction of reaction shift at different value of the reaction quotient and the equilibrium constant.