Alright, let's solve the problem step-by-step to find the percentage yield.
1. Identify the actual yield and the theoretical yield:
- The actual yield is the amount of product actually collected from the reaction, which is [tex]\(125.4 \text{ grams of } C_3H_8\)[/tex].
- The theoretical yield is the amount of product that was expected to be produced if the reaction went perfectly, which is [tex]\(158.4 \text{ grams of } C_3H_8\)[/tex].
2. Write down the formula for percentage yield:
[tex]\[
\text{Percentage Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100
\][/tex]
3. Substitute the given values into the formula:
[tex]\[
\text{Percentage Yield} = \left( \frac{125.4}{158.4} \right) \times 100
\][/tex]
4. Perform the division:
[tex]\[
\frac{125.4}{158.4} \approx 0.7916666666666666
\][/tex]
5. Multiply by 100 to convert to a percentage:
[tex]\[
0.7916666666666666 \times 100 \approx 79.16666666666666 \%
\][/tex]
6. Finally, round to one decimal place if needed:
[tex]\[
79.2\%
\][/tex]
Hence, the percentage yield is approximately [tex]\(79.2\%\)[/tex].
Therefore, the correct answer is:
A. [tex]\( 79.2\% \)[/tex]
