QuestionMay 30, 2025

What is the percent yield of CO2 if 97.5 g of CO_(2) is collected? percent yield =underline ( )%

What is the percent yield of CO2 if 97.5 g of CO_(2) is collected? percent yield =underline ( )%
What is the percent yield of CO2 if 97.5 g of CO_(2) is collected? percent yield =underline ( )%

Solution
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Answer

Additional information needed for theoretical yield calculation. Explanation 1. Calculate Moles of CO_2 Use the formula: **moles = \frac{\text{mass}}{\text{molar mass}}**. The molar mass of CO_2 is 44.01 g/mol. Thus, moles of CO_2 = \frac{97.5 \, \text{g}}{44.01 \, \text{g/mol}}. 2. Determine Theoretical Yield This step requires additional information about the reaction to calculate the theoretical yield. Assuming a balanced equation and known reactants, calculate the expected moles of CO_2. 3. Calculate Percent Yield Use the formula: **percent yield = \left(\frac{\text{actual yield}}{\text{theoretical yield}}\right) \times 100\%**. Substitute the actual moles from Step 1 and theoretical moles from Step 2.

Explanation

1. Calculate Moles of $CO_2$<br /> Use the formula: **moles = \frac{\text{mass}}{\text{molar mass}}**. The molar mass of $CO_2$ is 44.01 g/mol. Thus, moles of $CO_2 = \frac{97.5 \, \text{g}}{44.01 \, \text{g/mol}}$.<br /><br />2. Determine Theoretical Yield<br /> This step requires additional information about the reaction to calculate the theoretical yield. Assuming a balanced equation and known reactants, calculate the expected moles of $CO_2$.<br /><br />3. Calculate Percent Yield<br /> Use the formula: **percent yield = \left(\frac{\text{actual yield}}{\text{theoretical yield}}\right) \times 100\%**. Substitute the actual moles from Step 1 and theoretical moles from Step 2.
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