Questions: Question 28 (1 point) A student ran the reaction below. They calculated a theoretical yield of HgCl2 to be 34.8 g. 2 KCl + Hg(NO3)2 --> HgCl2 + 2 KNO3 If the student actually collected 32.1 g after filtering and drying the precipitate, what is the percent yield for their experiment?

Question 28 (1 point) A student ran the reaction below. They calculated a theoretical yield of HgCl2 to be 34.8 g. 2 KCl + Hg(NO3)2 --> HgCl2 + 2 KNO3 If the student actually collected 32.1 g after filtering and drying the precipitate, what is the percent yield for their experiment?
Transcript text: Question 28 (1 point) A student ran the reaction below. They calculated a theoretical yield of $\mathrm{HgCl}_{2}$ to be 34.8 g . \[ 2 \mathrm{KCl}+\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2}-->\mathrm{HgCl}_{2}+2 \mathrm{KNO}_{3} \] If the student actually collected 32.1 g after filtering and drying the precipitate, what is the percent yield for their experiment? Your Answer: $\square$ $\square$ Answer units
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Solution

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Solution Steps

Step 1: Understand the Problem

The problem provides the theoretical yield of \(\mathrm{HgCl}_{2}\) as 34.8 g and the actual yield as 32.1 g. We need to calculate the percent yield of the reaction.

Step 2: Use the Percent Yield Formula

The percent yield is calculated using the formula: \[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\% \]

Step 3: Substitute the Given Values

Substitute the actual yield (32.1 g) and the theoretical yield (34.8 g) into the formula: \[ \text{Percent Yield} = \left( \frac{32.1}{34.8} \right) \times 100\% \]

Step 4: Calculate the Percent Yield

Perform the division and multiplication: \[ \text{Percent Yield} = \left( 0.9224 \right) \times 100\% = 92.24\% \]

Final Answer

The percent yield for the experiment is \(\boxed{92.24\%}\).

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