A) \[\Delta \,H>T\cdot \Delta \,S\]
B) \[\Delta \,H<T\cdot \Delta \,S\]
C) \[\Delta \,H=T\cdot \Delta \,S\]
D) \[T\cdot \Delta \,S=0\]
Correct Answer: B
Solution :
For a reaction, to be spontaneous, the value of \[\Delta G\] (i.e., free energy change) must negative. According to Gibbs-Helmholtz equation \[\Delta G=\Delta H-T\cdot \Delta S\] If reaction is endothermic \[(\Delta H=+ve),\]then \[\Delta G\] to be negative, \[T\cdot \Delta S>\Delta H\]
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