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For the question, enter the correct numerical value, (in decimal-notation, truncated/rounded-off to the second aecimal place, e.g., \( 6 \cdot 25,7 \cdot 00,-0 \cdot 33,-\cdot 30,30 \cdot 27,-127 \cdot 30 \) ) using the mouse and the onscreen virtual numeric keypad in the place designated to enter the answer.
The enthalpy of formation of hypothetical \( \mathrm{CaCl}(s) \) is theoretically found to be \( -188 \mathrm{~kJ} \mathrm{~mol}^{-1} \) and \( \Delta \mathrm{H}^{\circ} \) for \( \mathrm{CaCl}_{2}(s) \) is \( -795 \mathrm{~kJ} \mathrm{~mol}^{-1} \). Calculate \( \Delta_{f} \mathrm{H}^{\circ} \) (in \( \mathrm{kJ} \mathrm{mol}^{-1} \) ) for the disproportionation reaction.
\[
2 \mathrm{CaCl}(s) \longrightarrow \mathrm{CaCl}_{2}(s)+\mathrm{Ca}(s)
\]
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