Heat of reaction is defined as the amount of heat absorbed or evolved at a given temperaturewhen the reactants have combined to form the products is represented by a balanced chemcial equation. If the heat is denofed by q then the numerical value of q depends on the manner in which the reaction is performed for the two methods of conducting chemical reactions in calorimeters.
Constant volume W = 0 and `q_(v) = Delta E` Bomb calorimeter
Constant pressure W = – V `Delta`P, therefore `q_(P) = Delta E + P Delta V rar (V. Delta P)`
The heat capacity of a bomb calorimeter is 300 JK When 0.16 gm of methane was burnt in this calorimeter the temperature rose by `3^(@)`C. The value of `Delta`U per mole will be
A. 100 kJ
B. 90 kJ
C. 900 kJ
D. 48 kJ

Heat of reaction is defined as the amount of heat absorbed or evolved at a given temperaturewhen the reactants have combined to form the products is represented by a balanced chemcial equation. If the heat is denofed by q then the numerical value of q depends on the manner in which the reaction is performed for the two methods of conducting chemical reactions in calorimeters.
Constant volume W = 0 and `q_(v) = Delta E` Bomb calorimeter
Constant pressure W = – V `Delta`P, therefore `q_(P) = Delta E + P Delta V rar (V. Delta P)`
When maltose `C_(12)H_(22)O_(11)(s)` burns in a calorimetric bomb at 298 K yielding carbon dioxide and water, the heat of combustion is -1350 kcal/mol, the heat of combustion of maltose at constant pressure will be
A. `-2650` kcal/mol
B. `-675` kcal/mol
C. `-1350` kcal/mol
D. `-1100` kcal/mol