Question

The process in which an organic acid and an alcohol react to form an ester and water is known as esterification. Ethyl butanoate (C3H7COOC2H5) an ester is formed when the alcohol ethanol (C2H5OH) and butanoic acid (C3H7COOH) are heated in the presence of sulfuric acid.C2H5OH(l) + C3H7COOH(l) C3H7COOC2H5(l) + H2O(l)Determine the mass of ethyl butanoate produced if 6.00 mol of ethanol is used.

Answer 1

Esterification is a condensation reaction that forms an ester from an alcohol and a carboxylic acid. In this reaction, 6.00 mol of ethanol would produce 528.9 g of ethyl butanoate.

Step-by-step explanation:

Esterification is a condensation reaction in which an ester is formed from an alcohol and a carboxylic acid. In this specific reaction, ethanol and butanoic acid react to form ethyl butanoate and water.

The balanced equation for the reaction is: C2H5OH(l) + C3H7COOH(l) -> C3H7COOC2H5(l) + H2O(l)

To determine the mass of ethyl butanoate produced, you need to use the stoichiometry of the reaction. The molar ratio between ethanol and ethyl butanoate is 1:1. Therefore, if 6.00 mol of ethanol is used, the mass of ethyl butanoate produced would be the same, which is (6.00 mol)(88.15 g/mol) = 528.9 g.

Answer 2

697 g

Step-by-step explanation:

Ethanol (C₂H₅OH) and butanoic acid (C₃H₇COOH) react to form ethyl butanoate (C₃H₇COOC₂H₅) and water (H₂O).

C₂H₅OH + C₃H₇COOH → C₃H₇COOC₂H₅ + H₂O

The molar ratio of C₂H₅OH to C₃H₇COOC₂H₅ is 1:1. The moles of C₃H₇COOC₂H₅ produced from 6.00 moles of C₂H₅OH are:

6.00 mol C₂H₅OH × (1 mol C₃H₇COOC₂H₅/1 mol C₂H₅OH) = 6.00 mol C₃H₇COOC₂H₅

The molar mass of C₃H₇COOC₂H₅ is 116.16 g/mol. The mass corresponding to 6.00 mol is:

6.00 mol × (116.16 g/mol) = 697 g