Chemical reactions are invariably associated with the transfter of energy either in the form of heat or light. In the laboratory, heat changes in physical and chemical processes are measured with an instrument called calorimeter. Heat change in the process is calculated as
`{:(q = ms DeltaT,,s ="Specific heat"),(=cDeltaT,,c ="Heat capacity"):}`
Heat of reaction at constant volume is measured using bomb calorimeter.
`q_(V) = DeltaU =` Internal energy change
Heat of reaction at constant pressure is measured using simple or water calorimeter.
`q_(p) = DeltaH`
`q_(p) = q_(V) +P DeltaV`
`DeltaH = DeltaU +DeltanRT`
The heat capacity of a bomb calorimeter is `500 JK^(-1)`. When `0.1g` of methane was burnt in this calorimeter, the temperature rose by `2^(@)C`. The value of `DeltaU` per mole will be

Options

A. `+2 kJ`
B. `-2 kJ`
C. `+260 kJ`
D. `+160 kJ`