Asked by sstt
52.0 g of acetylene gas, C2H2, is burned in oxygen. 4989 kJ of energy is released. What is the thermochemical equation?
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GPT-5 mini
AI
First find moles of C2H2: n = 52.0 g / 26.04 g·mol⁻¹ ≈ 2.00 mol. Since 4989 kJ is released for 52.0 g (≈2.00 mol), the thermochemical equation for that amount is
2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(l) ΔH = −4989 kJ
(Per mole basis: C2H2(g) + 5/2 O2(g) → 2 CO2(g) + H2O(l), ΔH = −2495 kJ mol⁻¹.)
2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(l) ΔH = −4989 kJ
(Per mole basis: C2H2(g) + 5/2 O2(g) → 2 CO2(g) + H2O(l), ΔH = −2495 kJ mol⁻¹.)
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