The value of `DeltaE` for combustion of 16 g of `CH_4` is -885389 at 298 K. The `DeltaH` combustion for `CH_4` in `Jmol^(-1)` at this temperature will be : (Given that, `R = 8.314 JK^(-1) mol^(-1)`)

The combustion of benzene(/) gives CO_2(g) and H_2O(l) Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol^(-1) at 25^@C , heat of combustion (in kJ mol^(-1) ) of benzene at constant pressure will be (R = 8.314 JK^(-1) mol^(-1))

The combustion of benzene (l) gives CO_(2) (g) and H_(2)O (l) . Given that heat of combustion of benzene at constant volume is -3263.9 kJ * mol^(-1) at 25^(@) C , heat of combustion ( in kJ * mol^(-1)) of benzene at constant pressure will be - (R = 8.314 J * K^(-1) * mol^(-1) )