The heat of combustion of gaseous methane `(CH_(4))` at constant volume is measured in a bomb calorimeter at `298 K` and is found to be `-885.4 kJ mol^(-1)`.Find the value of enthalpy change.

Explanation

To find the enthalpy change (ΔH) for the combustion of methane (CH₄) at constant volume, we can follow these steps:

### Step 1: Understand the relationship between ΔH and ΔU
The relationship between the change in enthalpy (ΔH) and the change in internal energy (ΔU) is given by the equation:
\[ \Delta H = \Delta U + \Delta N_g RT \]
where:
- ΔU is the change in internal energy (which is the heat of combustion at constant volume),
- ΔN_g is the change in the number of moles of gas,
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