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

Options

A. `2C_(4)H_(10)(g)+130_(2)(g)to8CO_(2)(g)+10H_(2)O(l)`
`Delta_(c)H=-2658.0KJmol^(-1)`
B. `C_(4)H_(10)(g)+(13)/(2)O_(2)(g)to4CO_(2)(g)+5H_(2)O(g)`
`Delta_(c)H=-1329.0KJmol^(-1)`
C. `C_(4)H_(10)(g)+(13)/(2)O_(2)(g)to4CO_(2)(g)+5H_(2)O(l)`
`Delta_(c)H=-2658.0KJmol^(-1)`
D. `C_(4)H_(10)(g)+(13)/(2)O_(2)(g)to4CO_(2)(g)+5H_(2)O(l)`
`Delta_(c)H=-2658.0KJmol^(-1)`

Answer

c