A) \[\Delta H<T\Delta S\] reaction is exothermic and \[T\Delta S\] is + ve
B) \[\Delta H=-ve,\,T\Delta S=0\]
C) \[\Delta H=\,T\Delta S\]
D) \[\Delta H=-ve,\,\,T\Delta S=-ve\]
Correct Answer: A
Solution :
For a reaction to be spontaneous on the reaction at equilibrium: \[\Delta H=-ve\,\,\,\,\Delta S=+ve\] \[\Delta G=\Delta H-T\Delta S=-ve\] So, \[\Delta H<T\Delta S\], reaction is exothermic and \[T\Delta S\] is +ve statement is wrong.
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