Using the enthalpy changes shown below, $I_2(g) + 3\text{Cl}_2(g) \rightarrow 2\text{ICl}_3(s)$ $\Delta H^\circ = -214\ \text{kJ mol}^{-1}$ $I_2(s) \rightarrow I_2(g)$ $\Delta H^\circ = +38\ \text{kJ mol}^{-1}$ Calculate the standard enthalpy change of formation for iodine trichloride, $\text{ICl}_3(s)$?
- A$+176\ \text{kJ mol}^{-1}$
- B$-88\ \text{kJ mol}^{-1}$
- C$-176\ \text{kJ mol}^{-1}$
- D$-214\ \text{kJ mol}^{-1}$