In solid sulfur, the substance exists as molecules containing eight atoms joined by covalent bonds. For sulfur dioxide, the bonding arrangement is $\text{O}=\text{S}=\text{O}$. Enthalpy change of combustion of $\text{S}_8$, $\Delta H_c^\circ (\text{S}_8(s)) = -2376\,\text{kJ mol}^{-1}$. The energy needed to separate $1$ mole of $\text{S}_8(s)$ into gaseous atoms is $2232\,\text{kJ mol}^{-1}$. The $\text{O}=\text{O}$ bond enthalpy is $496\,\text{kJ mol}^{-1}$. Using 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$536\,\text{kJ mol}^{-1}$