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

During complete combustion of one mole of butane, 2658 kJ of heat is r

1.	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
Answer» During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is (a) $2 C_{4} H_{10} (g) + 13 O_{2} (g) \to 8 C O_{2} (g) + 10 H_{2} O (l); Δ_{c} H = - 2658.0 k J m o l^{- 1}$ (b) $C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l); Δ_{c} H = - 1329.0 k J m o l^{- 1}$ (c) $C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l); Δ_{c} H = - 2658.0 k J m o l^{- 1}$ (d) $C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l); Δ_{c} H = + 2658.0 k J m o l^{- 1}$