Question

suppose 3.5 g of compound a are consumed in a reaction with 9.5 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 6.4 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 of C

According to the law of conservation of mass, in a chemical reaction, the mass of reactants equals the mass of products.
The mass of reactants \(m = m(A)+m(B)\)
Given \(m(A) = 3.5\space g\) and \(m(B)=9.5\space g\)
\(m = 3.5 + 9.5=\boldsymbol{13.0\space g}\)

Step2: Calculate percent yield of C

The formula for percent yield is \(\text{Percent Yield}=\frac{\text{Actual Yield}}{\text{Theoretical Yield}}\times100\%\)
Given actual yield \(= 6.4\space g\) and theoretical yield \(=13.0\space g\)
\(\text{Percent Yield}=\frac{6.4}{13.0}\times 100\% \approx 49\%\)

Answer:

13.0 g
49%