Question

Given 8.50 g of butanoic acid and excess ethanol, how many grams of ethyl butyrate would be synthesized, assuming a complete 100% yield?

Answer 1

Ethyl butyrate is also more commonly known as the ethyl butanoate with chemical formula of C₆H₁₂O₂. The equation of the butanoic acid (C₄H₈O₂)  and ethanol (C₂H₆O) to form this substance can be written off as,
                            C₄H₈O₂ + C₂H₆O --> C₆H₁₂O₂ + H₂O
Note that the given equation is already balanced. Using dimensional analysis and conversion factors,
                (8.5 g C₄H₈O₂)(1 mol/88.11 g)(1 mol C₆H₁₂O₂/1 mol C₄H₈O₂)(116.16 g / mol)
                  =  112.06 grams of ethyl butyrate

ANSWER: 112. 06 grams
                  

Answer 2

Answer:

Amount of ethyl butyrate formed = 11.3 g

Explanation:

The reaction between butanoic acid (C3H7COOH) and excess ethanol (C2H5OH) is:

$C3H7COOH + C2H5OH \rightarrow C3H7COOC2H5 + H2O$

Since ethanol is the excess reagent, the formation of the product i.e. ethyl butyrate is influenced by the amount of butanoic acid present

Based on the reaction stoichiometry:

1 mole of butanoic acid produces 1 mole of ethyl butyrate

Mass of butanoic acid = 8.50 g

Molar mass of butanoic acid = 88 g/mol

$Moles\ of \ butanoic\ acid = \frac{Mass}{Molar\ mass} =\frac{8.50g}{88g/mol}=0.097 moles$

Moles of ethyl butyrate = 0.097

Molar mass of ethyl butyrate= 116 g/mol

$Mass\ of\ ethyl\ butyrate= 0.097*116 = 11.3 g$