Questions: In a certain chemical reaction Compound A combines with Compound B to produce Compound C (and no other products). Measurements were taken of the amounts of A and B present before and after a reaction that produced some C: Compound initial amount final amount A 1.5 g 0 g B 1.5 g 1.0 g 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 56%. Calculate the actual amount of C that was isolated at the end of the reaction. Round your answer to the nearest 0.1 g.

In a certain chemical reaction Compound A combines with Compound B to produce Compound C (and no other products). Measurements were taken of the amounts of A and B present before and after a reaction that produced some C:

Compound initial amount final amount
A 1.5 g 0 g
B 1.5 g 1.0 g

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 56%. Calculate the actual amount of C that was isolated at the end of the reaction. Round your answer to the nearest 0.1 g.

Transcript text: In a certain chemical reaction Compound A combines with Compound B to produce Compound C (and no other products). Measurements were taken of the 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 & 1.5 g & 0 g \\ \hline B & 1.5 g & 1.0 g \\ \hline \end{tabular} \begin{tabular}{|l|l|} \hline 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 $56 . \%$. Calculate \\ the actual amount of C that was isolated at the end of the reaction. \\ Round your answer to the nearest 0.1 g . \end{tabular}

Solution

Solution Steps

Step 1: Determine the Limiting Reactant

To find the theoretical yield of Compound C, we first need to determine the limiting reactant. From the data:

Initial amount of A = 1.5 g
Final amount of A = 0 g
Initial amount of B = 1.5 g
Final amount of B = 1.0 g

Compound A is completely consumed, while 0.5 g of Compound B is used. Therefore, Compound A is the limiting reactant.

Step 2: Calculate the Theoretical Yield of C

Assuming a 1:1 stoichiometry for simplicity (since no other information is provided), the entire mass of Compound A is converted to Compound C. Thus, the theoretical yield of C is equal to the initial mass of A, which is 1.5 g.

Step 3: Calculate the Actual Yield of C

The percent yield of C is given as 56%. The actual yield can be calculated using the formula:

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

Substituting the given values:

\[ \text{Actual Yield} = \left(\frac{56}{100}\right) \times 1.5 = 0.84 \, \text{g} \]

Rounding to the nearest 0.1 g, the actual yield is 0.8 g.