Question

in a certain chemical reaction compound a combines with compound b to produce compound c (and no other products). measuremen amounts of a and b present before and after a reaction that produced some c: \

$$\begin{tabular}{|c|c|c|} \\hline compound & initial amount & final amount \\\\ \\hline a & 6.0 g & 0 g \\\\ \\hline b & 9.5 g & 4.7 g \\\\ \\hline \\end{tabular}$$

calculate the theoretical yield of c. round your answer to the nearest 0.1 g. suppose the percent yield of c in this reaction was 51.%. calculate the actual amount of c that was isolated at the end of the reaction. round your answer to the nearest 0.1 g.

Explanation:

Step1: Find mass of A and B reacted

For A: Initial = 6.0 g, Final = 0 g. So mass of A reacted = \( 6.0 - 0 = 6.0 \) g.
For B: Initial = 9.5 g, Final = 4.7 g. Mass of B reacted = \( 9.5 - 4.7 = 4.8 \) g.

Step2: Calculate theoretical yield of C (Law of Conservation of Mass)

Total mass of reactants reacted = mass of A + mass of B = \( 6.0 + 4.8 = 10.8 \) g.
By conservation of mass, theoretical yield of C = 10.8 g.

Step3: Calculate actual yield (using percent yield)

Percent yield = \( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100\% \)
So, Actual Yield = \( \text{Theoretical Yield} \times \frac{\text{Percent Yield}}{100\%} \)
Substitute values: \( 10.8 \times \frac{51.}{100} = 10.8 \times 0.51 = 5.508 \approx 5.5 \) g.

Answer:

Theoretical yield of C: \( \boldsymbol{10.8} \) g
Actual amount of C: \( \boldsymbol{5.5} \) g