An alkene upon combustion produces `CO_(2)(g)"and"H_(2)O(g).` In this combustion process if there is no volume change, then, the no. of C atoms per molecule of alkene will be:

combustion gives CO_2(g) and H_2O(g) .Find ratio of number of atoms O to H in product formed.

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 JK–1 mol–1)

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 ?