During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is
(a) 2C₄H₁₀(g)+13O₂(g)→8CO₂(g)+10H₂O(l); ΔcH=−2658.0kJ mol⁻¹
(b) C₄H₁₀(g)+132O₂(g)→4CO₂(g)+5H₂O(l); ΔcH=−1329.0kJ mol⁻¹
(c) C₄H₁₀(g)+132O₂(g)→4CO₂(g)+5H₂O(l); ΔcH=−2658.0kJ mol⁻¹
(d) C₄H₁₀(g)+132O₂(g)→4CO₂(g)+5H₂O(l); ΔcH=+2658.0kJ mol⁻¹