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Gaseous methane 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 10.9 g of methane and 57.9 g of oxygen gas?rnrnround your answer to 3 significant figures.
Accepted Answer
The balanced chemical equation is:
CH₄ (g) + 2O₂ (g) → CO₂ (g) + 2H₂O (g)
1 mole of CH₄ reacts with 2 moles of O₂ to produce 1 mole of CO₂.
First, convert the mass of each reactant to moles:
moles of CH₄ = 10.9 g / 16.04 g/mol = 0.679 mol
moles of O₂ = 57.9 g / 32.00 g/mol = 1.81 mol
Determine the limiting reactant by comparing the mole ratio of the reactants to the stoichiometric ratio in the balanced chemical equation:
0.679 mol CH₄ / 1 = 0.679
1.81 mol O₂ / 2 = 0.905
CH₄ is the limiting reactant because its mole ratio is smaller than the stoichiometric ratio.
Calculate the theoretical yield of CO₂ using the stoichiometry of the balanced chemical equation:
moles of CO₂ = 0.679 mol CH₄ × (1 mol CO₂ / 1 mol CH₄) = 0.679 mol CO₂
Convert moles of CO₂ to grams:
mass of CO₂ = 0.679 mol CO₂ × 44.01 g/mol = 29.9 g CO₂
Therefore, the theoretical yield of CO₂ formed from the reaction of 10.9 g of methane and 57.9 g of oxygen gas is 29.9 g.
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