Practice question
Question
For the combustion of 16 g of methane at 298 K ( Δ Hc = -890.30 kJ/mol , molar mass = 16 g/mol), what is Δ U ? ( R = 8.314 J/mol·K )
Explanation
For CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(l) , Δ ng = 1 - 3 = -2 . Then, RT = 8.314 × 298 × 10⁻³ = 2.4776 kJ . Using Δ H = Δ U + Δ ng RT , Δ U = -890.30 - (-2 × 2.4776) = -890.30 + 4.9552 = -885.34 kJ/mol .
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