Question #b8b2b

2 Answers
Mar 3, 2015

This new yield will allow for the production of #"8.03 g"# of ethyl butyrate.

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

#"% yield" = "actual yield"/"theoretical yield" * 100#

Reearranging this equation to get the actual yield will result in

#"actual yield" = ("% yield" * "theoretical yield")/"100"#

#"actual yield" = (78.0 * "10.3 g")/"100" = "8.034 g"#

Rounded to three sig figs, the mass of ethyl butyrate produced will be

#m_("ethyl butyrate") = "8.03 g"#

Mar 7, 2015

We first calculate the molecular masses of butanoic acid and ethyl butanoate.

Butanoic acid #88.11# g/Mol
Ethyl butanoate #116.16# g/Mol

From the butanoic acid #78%=0.78*7.80=6.084g# is used

Now we work with ratios, because every 88.11g used will yield 116.16g


Answer: 8.02 grams of ethyl butanoate will be formed.