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

Options

A. `2C_(4)H_(10)(g) + 13O_(2)(g) to 8CO_(2)(g) + 10H_(2)O(l)`,
` Delta_(c)H = -2658.0 kJ "mol"^(-1)`
B. `C_(4)H_(10)(g) + 13/2O_(2)(g) to 4CO_(2)(g) + 5H_(2)O(g)`
`Delta_(c)H = -1329.0 kJ "mol"^(-1)`
C. `C_(4)H_(10)(g) + 13/2 O_(2)(g) to 4CO_(2)(g) + 5H_(2)O(l)`
`Delta_(c)H = -2658.0 kJ "mol"^(-1)`
D. `C_(4)H_(10)(g) + 13/2O_(2)(g) to 4CO_(2)(g) + 5H_(2)O(l)`
`Delta_(c)H = + 2658.0 kJ "mol"^(-1)`

Answer

C