For the reactions : `C(s) + O_(2) (g) to CO_(2) (g)`

Explanation

We are given that
`CH_(4) (g) + 2O_(2)(g) to CO_(2) (g) + 2H_(2)O(l)`
The internal energy change `(Delta U) = - 885.4` kj/mol = - 885400 j/mol
`Deltan_(g)=["Number or moles of gaseous products"]-["Number of moles of gaseous reactants"]`
= 1 - (1 + 2) = - 2 mol
T = 298 K, R = 8.134 `j K^(-1) mol^(-1)` Using the relation.
`Delta H = Delta U + Delta n_(g) RT = 885400j/mol+(-2) 8.314 j mol^(-1) K^(-1) xx 298 K`
= - `885400 j/mol - 4955 j/mol = - 890355 = - 890.355 kj/mol`