compound a reacts with compound b to form only one product, compound c, and its known the usual percent…

compound a reacts with compound b to form only one product, compound c, and its known the usual percent yield of c in this reaction is 76.%. suppose 1.5 g of a are reacted with excess compound b, and 3.0 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 its known the usual percent yield of c in this reaction is 76.%. suppose 1.5 g of a are reacted with excess compound b, and 3.0 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.

Answer

Explanation:

Step1: Recall percent - yield formula

Percent yield = $\frac{\text{Actual yield}}{\text{Theoretical yield}}\times100%$. We know the actual yield of C is 3.0 g and the percent yield is 76.0%. Let the theoretical yield of C be $x$. Then $76.0=\frac{3.0}{x}\times100$.

Step2: Solve for the theoretical yield $x$

First, rewrite the equation from Step 1 as $76.0x = 3.0\times100$. Then $x=\frac{3.0\times100}{76.0}\approx3.9$ g.

Since we are not given the balanced chemical equation to find the amount of B consumed, we cannot answer the second - part of the question.

Answer:

3.9 g