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)+13O_(2)(g)rarr8CO_(2)(g)+10H_(2)O(l)`
`Delta_(c)H=-2658.0kJmol^(-1)`
B. `C_(4)H_(10)(g)+(13)/(2)O_(2)(g)rarr4CO_(2)(g)+5H_(2)O(g)`
`Delta_(c)H=-1329.0kJmol^(-1)`
C. `C_(4)H_(10)(g)+(13)/(2)O_(2)(g)rarr4CO_(2)(g)+5H_(2)O(l)`
`Delta_(c)H=-2658.0kJmol^(-1)`
D. `C_(4)H_(10)(g)+(13)/(2)O_(2)(g)rarr4CO_(2)(g)+5H_(2)O(l)`
`Delta_(c)H=+2658.0kJmol^(-1)`

Answer

C

Explanation

Exothermic reaction for combustion of one mole of butane is represented as:
`C_(4)H_(6)(g)+(13)/(2)O_(2)(g)rarr4CO_(2)(g)+5H_(2)O(l)`
`Delta_(c)H=-2658kJmol^(-1)`