Question

suppose 7.5 g of compound a are consumed in a reaction with 10.0 g of compound b that produces only one product, compound c. calculate the theoretical yield of c. round your answer to the nearest 0.1 g. suppose 14.0 g of c are actually isolated at the end of the reaction. what is the percent yield of compound c? round your answer to the nearest whole percent.

Explanation:

Step1: Calculate theoretical yield

According to the law of conservation of mass, mass of reactants = mass of products.
Mass of \(A = 7.5\space g\), mass of \(B=10.0\space g\).
Theoretical yield of \(C=m(A)+m(B)=7.5 + 10.0=17.5\space g\)

Step2: Calculate percent yield

Percent yield formula: \(\text{Percent Yield}=\frac{\text{Actual Yield}}{\text{Theoretical Yield}}\times100\%\)
Actual yield of \(C = 14.0\space g\), theoretical yield of \(C = 17.5\space g\)
\(\text{Percent Yield}=\frac{14.0}{17.5}\times 100\% = 80\%\)

Answer:

17.5 g
80%