Answer:
According to Gibb's Helmholtz
equation: \[\Delta G=\Delta H-T\Delta S\]. Since entropy decreases as a result
of adsorption,\[\Delta S\] is -ve. Now, \[\Delta G\] i.e., free energy change
must be also -ve in case adsorption is to take place. At a given temperature,
if \[\Delta G\] is to be negative, then \[\Delta H\] must be negative. This
means that adsorption must be always exothermic in nature.
\[\underset{(-ve)}{\mathop{\Delta
G}}\,=\Delta H-\underset{(-ve)}{\mathop{T\Delta S}}\,\]
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