Questions: Compound A reacts with Compound B to form only one product, Compound C, and it's known the usual percent yield of C in this reaction is 69%. Suppose 9.5 g of A are reacted with excess Compound B, and 10.0 g of Compound C are successfully isolated at the end of the reaction. What was the theoretical yield of C? Round your answer to the nearest 0.1 g. How much B was consumed by the reaction? Round your answer to the nearest 0.1 g.

Compound A reacts with Compound B to form only one product, Compound C, and it's known the usual percent yield of C in this reaction is 69%. Suppose 9.5 g of A are reacted with excess Compound B, and 10.0 g of Compound C are successfully isolated at the end of the reaction. What was the theoretical yield of C? Round your answer to the nearest 0.1 g. How much B was consumed by the reaction? Round your answer to the nearest 0.1 g.
Transcript text: Compound A reacts with Compound B to form only one product, Compound C, and it's known the usual percent yield of C in this reaction is $69 . \%$. Suppose 9.5 g of A are reacted with excess Compound B , and 10.0 g of Compound C are successfully isolated at the end of the reaction. What was the theoretical yield of C ? Round your answer to the nearest 0.1 g . $\square$ $\square$ 10 $\mu$ How much B was consumed by the reaction? $\cdot$ Round your answer to the nearest 0.1 g . $\square$
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Solution

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Solution Steps

Step 1: Understanding the Problem

We are given that Compound A reacts with Compound B to form Compound C with a percent yield of 69%. We need to find the theoretical yield of Compound C when 9.5 g of A is reacted with excess B, and 10.0 g of C is isolated.

Step 2: Calculate Theoretical Yield

The percent yield formula is given by:

\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\% \]

We know the percent yield is 69% and the actual yield is 10.0 g. We can rearrange the formula to solve for the theoretical yield:

\[ \text{Theoretical Yield} = \frac{\text{Actual Yield}}{\text{Percent Yield}} \times 100\% \]

Substituting the known values:

\[ \text{Theoretical Yield} = \frac{10.0 \, \text{g}}{69\%} \times 100\% = \frac{10.0 \, \text{g}}{0.69} \approx 14.4928 \, \text{g} \]

Rounding to the nearest 0.1 g, the theoretical yield is 14.5 g.

Step 3: Calculate Amount of B Consumed

Since we are not given the stoichiometry of the reaction, we cannot directly calculate the amount of B consumed without additional information such as the balanced chemical equation or molar masses. Therefore, this part of the question cannot be answered with the given data.

Final Answer

  • The theoretical yield of Compound C is \(\boxed{14.5 \, \text{g}}\).
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