In solid sulfur, the molecules are each formed from eight atoms linked by covalent bonds. In sulfur dioxide, the bonding is $\text{O}=\text{S}=\text{O}$. The 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 $1.0\,\text{mol}$ $\text{S}_8(s)$ into gaseous atoms is $2232\,\text{kJ mol}^{-1}$. The $\text{O}=\text{O}$ bond enthalpy is $496\,\text{kJ mol}^{-1}$. From these data, determine 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$536\,\text{kJ mol}^{-1}$