A) \[180\,\,kJ\,\,mo{{l}^{-1}}\]
B) \[360\,\,kJ\,\,mo{{l}^{-1}}\]
C) \[213\,\,kJ\,\,mo{{l}^{-1}}\]
D) \[425\,\,kJ\,\,mo{{l}^{-1}}\]
Correct Answer: D
Solution :
The formation of-one mole of \[HCl\] can be represented as, \[\frac{1}{2}(H-H)+\frac{1}{2}(Cl-Cl)\xrightarrow{{}}H-Cl;\] \[\Delta H=-90\,\,kJ\] Hence, for the reaction, Heat evolved = heat evolved in bond formation heat required for bond breaking \[\therefore \] \[90\,kJ=\] [\[H-Cl\] bond energy] \[-\left( \frac{1}{2}\times 430+\frac{1}{2}\times 24 \right)\] \[\therefore \] (\[HCl\] bond energy) \[=90+\text{(}215+120\text{)}\] \[=\text{ }425\text{ }kJ\,\,mo{{l}^{-1}}\].
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