Question

In completing a Fischer Esterification experiment using acetic acid and unknown alcohol catalyzed by sulfuric acid a student starts with excess acetic acid with the intention of shifting the equilibrium towards formation of product. Identify the law used to predict this effect.

Answer 1

LeChatelier's principle is used to predict the effect of shifting the equilibrium towards the formation of product in a Fischer Esterification experiment with excess acetic acid.

Step-by-step explanation:

The law used to predict the effect of shifting the equilibrium towards the formation of product in a Fischer Esterification experiment is LeChatelier's principle. According to LeChatelier's principle, when a system at equilibrium is subjected to a change in conditions, it will shift in a direction that minimizes the effect of the change. In this case, starting with excess acetic acid will shift the equilibrium towards the formation of ethyl acetate, the desired product.The Law of Mass Action is used to predict the shift of an equilibrium upon changing the concentrations of reactants or products. In the case of the Fischer esterification experiment, using excess acetic acid increases the concentration of the reactants, thereby driving the reaction towards the formation of more ester product.

Answer 2

The equilibrium law

Step-by-step explanation:

According to the equilibrium law , when
`$\text{concentration}$` of any of the reactants or the products in the reaction at an equilibrium state, is changed, then it changes the composition of equilibrium mixture in order to minimize the effect of

Acetic acid (in excess) +
`$\text{alcohol}$` ⇄
`$\text{ester}$` + water

`$\text{Fischer esterification}$` is a reaction which involves the equilibrium. So to force the reaction towards the side of
`$\text{ester}$`, one of the reactant is taken in excess. All this can be explained easily by applying the equilibrium law.