If 1.00 g CH4 is combusted, how many grams of CO2 are theoretically produced? (CH4 + 2 O2 → CO2 + 2 H2O; M_CH4 = 16.04 g/mol; M_CO2 = 44.01 g/mol)

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Multiple Choice

If 1.00 g CH4 is combusted, how many grams of CO2 are theoretically produced? (CH4 + 2 O2 → CO2 + 2 H2O; M_CH4 = 16.04 g/mol; M_CO2 = 44.01 g/mol)

Explanation:
This problem uses stoichiometry to relate the mass of methane to the mass of carbon dioxide produced in complete combustion. From the balanced equation, one mole of methane yields one mole of carbon dioxide, so the moles of CO2 produced equal the moles of CH4 that react. Convert the given methane mass to moles: 1.00 g CH4 × (1 mol CH4 / 16.04 g CH4) ≈ 0.0623 mol CH4. Thus, the same amount in moles of CO2 is produced: 0.0623 mol CO2. Convert moles CO2 to mass: 0.0623 mol × 44.01 g CO2/mol ≈ 2.74 g CO2. Rounding gives about 2.75 g. So about 2.75 g of CO2 would be produced.

This problem uses stoichiometry to relate the mass of methane to the mass of carbon dioxide produced in complete combustion. From the balanced equation, one mole of methane yields one mole of carbon dioxide, so the moles of CO2 produced equal the moles of CH4 that react.

Convert the given methane mass to moles: 1.00 g CH4 × (1 mol CH4 / 16.04 g CH4) ≈ 0.0623 mol CH4.

Thus, the same amount in moles of CO2 is produced: 0.0623 mol CO2.

Convert moles CO2 to mass: 0.0623 mol × 44.01 g CO2/mol ≈ 2.74 g CO2. Rounding gives about 2.75 g.

So about 2.75 g of CO2 would be produced.

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