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Answer :
To determine the percent yield of a chemical reaction, we use the following formula:
[tex]\[
\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100
\][/tex]
Here's a step-by-step breakdown of the calculation:
1. Identify the theoretical yield:
The theoretical yield is the maximum amount of product that can be formed from the given amounts of reactants under ideal conditions. In this problem, the theoretical yield of lead(II) carbonate (PbCO[tex]\(_3\)[/tex]) is given as 63.3 grams.
2. Identify the actual yield:
The actual yield is the amount of product that is actually recovered from the reaction. In this problem, the actual yield of lead(II) carbonate is 36.3 grams.
3. Plug these values into the percent yield formula:
[tex]\[
\text{Percent Yield} = \left( \frac{36.3 \text{ grams}}{63.3 \text{ grams}} \right) \times 100
\][/tex]
4. Calculate the division:
[tex]\[
\frac{36.3}{63.3} \approx 0.5734597156398104
\][/tex]
5. Multiply by 100 to get the percent yield:
[tex]\[
0.5734597156398104 \times 100 \approx 57.34597156398104
\][/tex]
6. Round to an appropriate number of significant figures (if necessary):
Depending on the precision required, you might round the result. For this problem, let's report the percent yield to two decimal places:
[tex]\[
\text{Percent Yield} \approx 57.35\%
\][/tex]
So, the percent yield of lead(II) carbonate in this reaction is approximately 57.35%.
[tex]\[
\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100
\][/tex]
Here's a step-by-step breakdown of the calculation:
1. Identify the theoretical yield:
The theoretical yield is the maximum amount of product that can be formed from the given amounts of reactants under ideal conditions. In this problem, the theoretical yield of lead(II) carbonate (PbCO[tex]\(_3\)[/tex]) is given as 63.3 grams.
2. Identify the actual yield:
The actual yield is the amount of product that is actually recovered from the reaction. In this problem, the actual yield of lead(II) carbonate is 36.3 grams.
3. Plug these values into the percent yield formula:
[tex]\[
\text{Percent Yield} = \left( \frac{36.3 \text{ grams}}{63.3 \text{ grams}} \right) \times 100
\][/tex]
4. Calculate the division:
[tex]\[
\frac{36.3}{63.3} \approx 0.5734597156398104
\][/tex]
5. Multiply by 100 to get the percent yield:
[tex]\[
0.5734597156398104 \times 100 \approx 57.34597156398104
\][/tex]
6. Round to an appropriate number of significant figures (if necessary):
Depending on the precision required, you might round the result. For this problem, let's report the percent yield to two decimal places:
[tex]\[
\text{Percent Yield} \approx 57.35\%
\][/tex]
So, the percent yield of lead(II) carbonate in this reaction is approximately 57.35%.
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