A) - 767 kJ/mol
B) 767 kJ/mol
C) -392 kJ/mol
D) 392 kJ/mol
Correct Answer: C
Solution :
\[Mg(s)+C{{l}_{2}}(g)\xrightarrow{{}}MgC{{l}_{2}}(s)\], \[\Delta {{H}_{1}}=-642\,\,kJ/mole\] \[Mg(s)+\frac{1}{2}C{{l}_{2}}(g)\xrightarrow{{}}MgCl(s)\], \[\Delta {{H}_{2}}=-125\,kJ/mol\] \[2MgCl\xrightarrow{_{{}}}MgC{{l}_{2}}+Mg\], \[\Delta H=?\] \[\Delta H=\Delta {{H}_{1}}-2\Delta {{H}_{2}}\] \[=-642-2\times (-125)\] \[=-392\,kJ/mol\]You need to login to perform this action.
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