The heat of combustion of `H_(2)(g)` at constant pressure and `300k` is `-280kJ mol^(-1)`. What will be the heat of combustion at constant volume and at `300K`?

Explanation

To find the heat of combustion of \( H_2(g) \) at constant volume, we can use the relationship between the heat of combustion at constant pressure (\( \Delta H \)) and at constant volume (\( \Delta U \)). The relationship is given by:

\[ \Delta H = \Delta U + \Delta N_g R T \]

Where:
- \( \Delta H \) is the heat of combustion at constant pressure.
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