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What mass of methane is required to produce 1.130 kg of carbon dioxide during combustion? (assume the reaction undergoes complete combustion.) question 16 options: 41.18 g 4.118 g 0.4118 g 411.8 g
Accepted Answer
Here's how to solve this problem:
1. Balanced Chemical Equation:
The combustion of methane (CH₄) produces carbon dioxide (CO₂) and water (H₂O):
CH₄ + 2O₂ → CO₂ + 2H₂O
2. Stoichiometry:
The balanced equation shows that 1 mole of CH₄ reacts to produce 1 mole of CO₂.
3. Convert Mass to Moles:
Molar mass of CO₂ = 44.01 g/mol
Moles of CO₂ = (1.130 kg CO₂)
(1000 g/kg) / (44.01 g/mol) = 25.68 mol CO₂
4. Calculate Moles of CH₄:
Since the mole ratio is 1:1, 25.68 mol of CO₂ requires 25.68 mol of CH₄.
5. Convert Moles to Mass:
Molar mass of CH₄ = 16.04 g/mol
Mass of CH₄ = (25.68 mol CH₄)
(16.04 g/mol) = 411.8 g CH₄
Therefore, the mass of methane required is 411.8 g.
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