In solid sulfur, the particles are molecules containing eight atoms joined together by covalent bonds. In sulfur dioxide, the bonding arrangement is $\text{O}=\text{S}=\text{O}$. Information: - Enthalpy change of combustion of $\text{S}_8$, $\Delta H_c^\circ(\text{S}_8(s)) = -2376\,\text{kJ mol}^{-1}$ - Energy needed to separate $1$ mole $\text{S}_8(s)$ into gaseous atoms $= 2232\,\text{kJ mol}^{-1}$ - $\text{O}=\text{O}$ bond enthalpy $= 496\,\text{kJ mol}^{-1}$ From these data, what is the value of the $\text{S}=\text{O}$ bond enthalpy?
- A$239\,\text{kJ mol}^{-1}$
- B$257\,\text{kJ mol}^{-1}$
- C$319\,\text{kJ mol}^{-1}$
- D$536\,\text{kJ mol}^{-1}$