InterviewSolution
Saved Bookmarks
InterviewSolution
| 1. |
During complete combustion of one mole of butane, 2658kJ of heat is released. The thermochemical reaction for above changeisA. `2C_(4)H_(10)(g)+13O_(2)(g) rarr 8 CO_(2)(g) +10 H_(2)O(l) Delta_(c) H=- 2658.0 kJ mol^(-1)`B. `C_(4)H_(10)(g)+ (13)/(2) O_(2)(g) rarr4CO_(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) rarr4CO_(2)(g)+5H_(2)O(l) Delta_(c)H=- 2658.0 kJ mol^(-1)`D. `C_(4)H_(10)(g)+ (13)/(2) O_(2)(g) rarr4CO_(2)(g)+5H_(2)O(l) Delta_(c)H=+ 2658.0 kJ mol^(-1)` |
|
Answer» Correct Answer - c We have to take the combustion of one mole of `C_(4)H_(10)` and `Delta_(c) H` should be `-ve` and have a value of 2658 kJ mol`^(-1)` |
|