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(B) Adsorption is an exothermic process,therefore the enthalpy change is negative $(\Delta H < 0)$.Furthermore,adsorption leads to a more ordered arra

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$\Delta H < 0$ and $\Delta S < 0$

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(B) Adsorption is an exothermic process,therefore the enthalpy change is negative $(\Delta H Furthermore,adsorption leads to a more ordered arrangement of gas molecules on the surface,resulting in a decrease in entropy $(\Delta S According to the Gibbs free energy equation,$\Delta G = \Delta H - T\Delta S$,the process is spontaneous when $\Delta G < 0$,which is favored at low temperatures.

During the adsorption of krypton on activated charcoal at low temperature,

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