Preparing Isopentyl Acetate: Why Extra Acetic Acid is Needed

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SUMMARY

The preparation of isopentyl acetate necessitates the use of a large excess of acetic acid due to its cost-effectiveness compared to isopentyl alcohol. This approach leverages Le Chatelier's principle, which states that an increase in the concentration of a reactant shifts the equilibrium of the reaction towards the products. By using excess acetic acid, the equilibrium is driven to favor the formation of isopentyl acetate, thereby enhancing the yield of the esterification reaction.

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Why is it necessary to use a large excess of acetic adic in the prepartion of isopentyl acetate?
 
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You can do this in another way, but acetic acid is far more cheap than isopentyl alcohol. This is just for being more economical.

If you've heard what Le Chatelier's principle is, it will make more sense. Esterification reactions require removal of water, so using one of the reactants in excess will drive the reaction to the ester side. So, what reactant would you use?
 
The excess of acetic acid is used to shift the equilibrium to the right so more isopentyl acetate is produced.
 

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