This new yield will allow for the production of
Since this question builds upon what was already solved here
I'll skip the balanced chemical equation and the theoretical yield and just show you how to get the new mass produced.
So, the theoretical yield for 7.80 g of butanoic acid was calculated at 10.3 g. When the reaction had a percent yield of 54.9%, only 5,65 g were produced.
It is safe to assume that the new yield of 78.0% will allow for the production of more ethyl butyrate. To determine this new mass, use the definition of the percent yield
Reearranging this equation to get the actual yield will result in
Rounded to three sig figs, the mass of ethyl butyrate produced will be
We first calculate the molecular masses of butanoic acid and ethyl butanoate.
From the butanoic acid
Now we work with ratios, because every 88.11g used will yield 116.16g
Answer: 8.02 grams of ethyl butanoate will be formed.