A) \[180\,\text{kJmo}{{\text{l}}^{-1}}\]
B) \[360\,\text{kJmo}{{\text{l}}^{-1}}\]
C) \[213\,\text{kJ}\,\text{mo}{{\text{l}}^{-1}}\]
D) \[425\,\text{kJ}\,\text{mo}{{\text{l}}^{-}}\]
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] \[-\left( \frac{1}{2}\times 430\times \frac{1}{2}\times 240 \right)\] \[\therefore \] (\[H-Cl\] bond energy) = 90 + (215 + 120) \[=425\,\text{kJ}\,\text{mo}{{\text{l}}^{-1}}\]You need to login to perform this action.
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