Heat of combustion of `CH_4`(g) at constant volume and at 298 K has been found to be -`885 kJ mol^(-1)`, calculate the enthalpy of its combustion under constant pressure condition (`R = 8.31 J K^(-1) mol^(-1)`).

Explanation

To calculate the enthalpy of combustion of methane (CH₄) under constant pressure conditions, we can use the relationship between the internal energy change (ΔE) and the enthalpy change (ΔH). The formula we will use is:

\[ \Delta H = \Delta E + \Delta N_g \cdot R \cdot T \]

Where:
- ΔH = Enthalpy change
...