A) \[180\text{ }kJ\text{ }mo{{l}^{-1}}\]
B) \[360\text{ }kJ\text{ }mo{{l}^{-1}}\]
C) \[\text{213 }kJ\text{ }mo{{l}^{-1}}\]
D) \[\text{425 }kJ\text{ }mo{{l}^{-1}}\]
Correct Answer: D
Solution :
The formation of one mole of \[HCl\] can be represented as, \[\frac{1}{2}(H-H)+\frac{1}{2}(Cl-Cl)\xrightarrow{{}}H-Cl;\]\[\Delta H=-90kJ\] Hence, for the reaction, Heat evolved = Heat evolved in bond formation - Heat required for bond-breaking \[\therefore \] \[90kJ=\] [\[H-Cl\] bond energy] \[-\left( \frac{1}{2}\times 430+\frac{1}{2}\times 240 \right)\] \[\therefore \] (\[H-Cl\] bond energy) \[=90+(215+120)\] \[=425kJmo{{l}^{-1}}\]
You need to login to perform this action.
You will be redirected in
3 sec
