During complete combustion of one mole of butane, 2658 kJ of heat i...

During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is

A. \(2\mathrm{C_4H_{10}(g) + 13O_2(g)\rightarrow 8CO_2(g) + 10H_2O(l)}; \Delta_c H = -2658.0\mathrm{kJmol^{-1}}\)

B. \(\mathrm{C_4H_{10}(g) + \frac{13}{2}O_2(g)\rightarrow 4CO_2(g) + 5H_2O(g)}; \Delta_c H = -1329.0\mathrm{kJmol^{-1}}\)

C. \(\mathrm{C_4H_{10}(g) + \frac{13}{2}O_2(g)\rightarrow 4CO_2(g) + 5H_2O(l)}; \Delta_c H = -2658.0\mathrm{kJmol^{-1}}\)

D. \(\mathrm{C_4H_{10}(g) + \frac{13}{2}O_2(g)\rightarrow 4CO_2(g) + 5H_2O(l)}; \Delta_c H = +2658.0\mathrm{kJmol^{-1}}\)