Final answer:
The percent yield can be calculated by dividing the actual yield by the theoretical yield and multiplying by 100. In this case, the percent yield is 70.37%. So, option C is correct.
Step-by-step explanation:
The percent yield can be calculated by dividing the actual yield (5.70 g of ethyl butyrate) by the theoretical yield (the maximum amount of ethyl butyrate that could be formed from the given amount of butanoic acid) and multiplying by 100.
To calculate the theoretical yield, we need to determine the limiting reactant. In this case, butanoic acid is the limiting reactant because it is used up completely, while ethanol is in excess. The balanced chemical equation for the reaction is:
C₄H₈O₂ + C₂H₅OH → C₆H₁₂O₂ + H₂O
The molar mass of butanoic acid is 88.11 g/mol and the molar mass of ethyl butyrate is 116.16 g/mol. Using the mole ratio from the balanced equation, we can calculate the theoretical yield of ethyl butyrate:
Theoretical yield = (8.10 g / 88.11 g/mol) * (116.16 g/mol / 1 mol) = 9.47 g
Now we can calculate the percent yield:
Percent yield = (5.70 g / 9.47 g) * 100 = 70.37%