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Gaseous butane reacts with gaseous oxygen gas to produce gaseous carbon dioxide and gaseous water . What is the theoretical yield of carbon dioxide formed from the reaction of 9.88 g of butane and 61.5 g of oxygen gas?rnrnround your answer to 3 significant figures.
Accepted Answer
1. Write a balanced chemical equation for the combustion of butane:
C4H10 + 6.5O2 → 4 CO2 + 5 H2O
2. Convert the masses of butane and oxygen gas to moles:
moles of C4H10 = 9.88 g / 58.12 g/mol = 0.170 mol
moles of O2 = 61.5 g / 32.00 g/mol = 1.92 mol
3. Determine the limiting reactant by comparing the moles of each reactant to the stoichiometric coefficients in the balanced equation. The reactant that produces the fewest moles of product is the limiting reactant.
moles of CO2 from C4H10 = 0.170 mol C4H10 × 4 mol CO2 / 1 mol C4H10 = 0.680 mol CO2
moles of CO2 from O2 = 1.92 mol O2 × 4 mol CO2 / 6.5 mol O2 = 1.19 mol CO2
Since C4H10 produces fewer moles of CO2, it is the limiting reactant.
4. Calculate the theoretical yield of carbon dioxide using the stoichiometry of the balanced equation and the moles of the limiting reactant:
moles of CO2 = 0.170 mol C4H10 × 4 mol CO2 / 1 mol C4H10 = 0.680 mol CO2
5. Convert the moles of carbon dioxide to grams:
mass of CO2 = 0.680 mol CO2 × 44.01 g/mol = 30.0 g CO2
Therefore, the theoretical yield of carbon dioxide formed from the reaction of 9.88 g of butane and 61.5 g of oxygen gas is 30.0 g.
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