QuestionJuly 5, 2025

3. For the balanced equation shown below, if the reaction of 91.39 grams of C_(3)H_(6) produces a 81.36% yield, how many grams of CO_(2) would be produced? 2C_(3)H_(6)+9O_(2)Longrightarrow 6CO_(2)+6H_(2)O

3. For the balanced equation shown below, if the reaction of 91.39 grams of C_(3)H_(6) produces a 81.36% yield, how many grams of CO_(2) would be produced? 2C_(3)H_(6)+9O_(2)Longrightarrow 6CO_(2)+6H_(2)O
3. For the balanced equation shown below, if the reaction of 91.39 grams of C_(3)H_(6) produces a 81.36% yield, how many grams of CO_(2) would be produced? 2C_(3)H_(6)+9O_(2)Longrightarrow 6CO_(2)+6H_(2)O

Solution
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Answer

233.47 g of CO_2 would be produced. Explanation 1. Calculate Molar Mass of C_3H_6 Molar mass of C_3H_6 = 3(12.01) + 6(1.01) = 42.08 \, \text{g/mol}. 2. Calculate Moles of C_3H_6 Moles of C_3H_6 = \frac{91.39 \, \text{g}}{42.08 \, \text{g/mol}} = 2.172 \, \text{mol}. 3. Determine Moles of CO_2 Produced From the balanced equation, 2 \, \text{mol} \, C_3H_6 produces 6 \, \text{mol} \, CO_2. Therefore, 2.172 \, \text{mol} \, C_3H_6 produces \frac{6}{2} \times 2.172 = 6.516 \, \text{mol} \, CO_2. 4. Calculate Theoretical Mass of CO_2 Molar mass of CO_2 = 12.01 + 2(16.00) = 44.01 \, \text{g/mol}. Thus, theoretical mass of CO_2 = 6.516 \, \text{mol} \times 44.01 \, \text{g/mol} = 286.77 \, \text{g}. 5. Calculate Actual Yield of CO_2 Actual yield = 81.36\% \times 286.77 \, \text{g} = 0.8136 \times 286.77 \, \text{g} = 233.47 \, \text{g}.

Explanation

1. Calculate Molar Mass of $C_3H_6$<br /> Molar mass of $C_3H_6 = 3(12.01) + 6(1.01) = 42.08 \, \text{g/mol}$.<br /><br />2. Calculate Moles of $C_3H_6$<br /> Moles of $C_3H_6 = \frac{91.39 \, \text{g}}{42.08 \, \text{g/mol}} = 2.172 \, \text{mol}$.<br /><br />3. Determine Moles of $CO_2$ Produced<br /> From the balanced equation, $2 \, \text{mol} \, C_3H_6$ produces $6 \, \text{mol} \, CO_2$. Therefore, $2.172 \, \text{mol} \, C_3H_6$ produces $\frac{6}{2} \times 2.172 = 6.516 \, \text{mol} \, CO_2$.<br /><br />4. Calculate Theoretical Mass of $CO_2$<br /> Molar mass of $CO_2 = 12.01 + 2(16.00) = 44.01 \, \text{g/mol}$. Thus, theoretical mass of $CO_2 = 6.516 \, \text{mol} \times 44.01 \, \text{g/mol} = 286.77 \, \text{g}$.<br /><br />5. Calculate Actual Yield of $CO_2$<br /> Actual yield = $81.36\% \times 286.77 \, \text{g} = 0.8136 \times 286.77 \, \text{g} = 233.47 \, \text{g}$.
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