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