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Gaseous butane reacts with gaseous oxygen gas to produce gaseous carbon dioxide and gaseous water . if 4.63 g of carbon dioxide is produced from the reaction of 1.7 g of butane and 9.7 g of oxygen gas, calculate the percent yield of carbon dioxide. round your answer to 2 significant figures.
Accepted Answer
Here's how to calculate the percent yield of carbon dioxide:
1. Balanced Chemical Equation:
C4H10(g) + 13/2 O2(g) → 4 CO2(g) + 5 H2O(g)
2. Calculate the Theoretical Yield:
Convert grams of butane to moles: 1.7 g C4H10
(1 mol C4H10 / 58.12 g C4H10) = 0.0292 mol C4H10
Use the mole ratio from the balanced equation to find moles of CO2: 0.0292 mol C4H10
(4 mol CO2 / 1 mol C4H10) = 0.117 mol CO2
Convert moles of CO2 to grams: 0.117 mol CO2
(44.01 g CO2 / 1 mol CO2) = 5.15 g CO2 (theoretical yield)
3. Calculate the Percent Yield:
Percent Yield = (Actual Yield / Theoretical Yield)
100%
Percent Yield = (4.63 g CO2 / 5.15 g CO2)
100% = 89.9%
Therefore, the percent yield of carbon dioxide is approximately 90%.
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