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To solve this problem, let’s analyze the information provided and calculate the percentage yield.

**Given dataTo solve this problem, let’s analyze the information provided and calculate the percentage yield.

**Given **
- The theoretical yield (the amount of \( CO_2 \) expected to be produced if the reaction went perfectly) is \( 29.9 \, \text{kg} \).
- The actual yield (the amount of \( CO_2 \) actually produced) is \( 27.3 \, \text{kg} \).

**Formula for percentage yield:**

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

**Substitute the values:**

\[
\text{Percentage yield} = \left( \frac{27.3}{29.9} \right) \times 100
\]

Calculating this:

\[
\text{Percentage yield} = \left( 0.9130 \right) \times 100 = 91.30\%
\]

**Answer:** The percentage yield is approximately \( 91.3\% \).

Would you like a deeper explanation on any steps or additional questions? Here are some related questions to consider:

1. How would the yield calculation change if only partial data was provided?
2. What factors can lead to a yield being less than 100% in real reactions?
3. How is theoretical yield determined in practice, especially in complex reactions?
4. Why is percentage yield important in industrial and chemical processes?
5. Could other forms of yield (like atom economy) be useful in this context?

**Tip:** To improve yield in experiments, it’s important to optimize reaction conditions, minimize product loss, and control side reactions.

A 10kg bottle of LPG gas should yield 29.9kg of CO2. Only 27.3kg of CO2 were produced. What is the percentage yield?

Learn how to calculate the percentage yield of CO2 when only 27.3kg is produced from an LPG gas reaction that theoretically yields 29.9kg. This problem covers key concepts like percentage yield and ratios, suitable for students in Grades 9-12.

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