Question

Although ${\mathbf{K}}_{\mathbf{eq}}$of Equation [1] in Problem 6.57 does not greatly favor formation of the product, it is sometimes possible to use Le Châtelier’s principle to increase the yield of ethyl acetate. Le Châtelier’s principle states that if an equilibrium is disturbed, a system will react to counteract this disturbance. How can Le Châtelier’s principle be used to drive the equilibrium to increase the yield of ethyl acetate? Another example of Le Châtelier’s principle is given in Section 9.8

Short answer

Answer

Increasing the concentration of acetic acid or ethanol leads to an increase in the yield of ethyl acetate.

Step-by-step solution

Step-by-Step SolutionStep 1: Le-Chatelier’s principle

Le Chatelier’s principle is used to describe the effect of changes in an equilibrium reaction.

It states that any change created on a system in equilibrium leads to the shift of reaction in a direction opposite to the change such that the induced change is neutralized.

The reaction of acetic acid with ethanol

The reaction of acetic acid with ethanol yields ethyl acetate.

Esterification reaction

Applying Le Chatelier’s principle to increase the yield

The increase in the concentration of the reactants leads to an increase in the concentration of the products as the reaction proceeds forwards to neutralize/counteract the increase in the concentration of the reactant.

Therefore, increasing the concentration of acetic acid or ethanol leads to an increase in the yield of ethyl acetate.