A) \[223.18\,kJ\,mo{{l}^{-1}}\]
B) \[423.38\,kJ\,mo{{l}^{-1}}\]
C) \[513.28\,kJ\,mo{{l}^{-1}}\]
D) \[113.38\,kJ\,mo{{l}^{-1}}\]
Correct Answer: B
Solution :
[b] We have to calculate the enthalpy of the reaction \[OH\,(g)\to O\,(g)+H\,(g)\] From the given reactions, this can be obtained as follows. \[-\left[ \frac{1}{2}{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\to OH(g) \right];\]\[\Delta H=-42.09\,kJ\,\,mo{{l}^{-1}}\] \[+\frac{1}{2}[{{H}_{2}}(g)\to 2H(g)];\]\[\Delta H=\frac{1}{2}\times 435.89\,kJ\,\,mo{{l}^{-1}}\] \[+\frac{1}{2}[{{O}_{2}}(g)\to 2O(g)];\]\[\Delta H=\frac{1}{2}\times 495.05\,kJ\,\,mo{{l}^{-1}}\] Add \[\overset{{}}{\mathop{\overline{OH(g)\to H(g)+O(g)}}}\,\,\,\,;\]\[\Delta H=\]\[\overline{423.38\,\,kJ\,\,mo{{l}^{-1}}}\]You need to login to perform this action.
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