Using the provided data, calculate the enthalpy change ($$\Delta H) $$for the formation of LiCl(s) from its elements in their standard states: $$\mathrm{Li(s) + \frac{1}{2}Cl_2$(g) \rightarrow LiCl(s)}. $$Which of the following is the correct value?

Question

Accepted Answer

$$\Delta H = -408.3\ \mathrm{kJ/mol}$$

Calculating the Energy Change for Formation of LiCl(s) Using Hess's Law

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