128 grams of rhombic sulphur when burnt in excess of oxygen liberated Q kJ of heat. Enthalpy of combustion of rhombic sulphur is -------------- kJ/mole

$$\begin{gathered} \mathrm{Rhombic} \mathrm{sulphur} \mathrm{is} {\mathrm{S}}_8. \\ {\mathrm{S}}_8+8{\mathrm{O}}_2 \to 8{\mathrm{SO}}_2; \\ 256 \mathrm{g} \mathrm{liberates} \mathrm{X} \mathrm{kJ} \\ 128 \mathrm{g} \mathrm{liberates} \mathrm{Q} \mathrm{kJ} \\ \mathrm{X}=2\mathrm{Q} \mathrm{kJ}; \\ \mathrm{One} \mathrm{mole} \mathrm{of} \mathrm{rhombic} \mathrm{sulphur} \mathrm{weighs} 256\mathrm{g} \\ \mathrm{Heat} \mathrm{liberated} \mathrm{by} \mathrm{the} \mathrm{combustion} \mathrm{of} \mathrm{one} \mathrm{mole} \mathrm{of} \mathrm{substance} \mathrm{is} \mathrm{Enthalpy} \mathrm{of} \mathrm{combustion}. \\ \mathrm{Thus}, {∆}^0{\mathrm{H}}_{\mathrm{c}}=-2\mathrm{Q} \mathrm{kJ} \end{gathered}$$