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Which of the following is true concerning adsorption?(A) $\Delta \text{G 0; }\Delta S\text{ 0; }\Delta H\text{ 0}$(B) $\Delta \text{G 0; }\Delta S\text{ 0; }\Delta H\text{ 0}$(C) $\Delta \text{G 0; }\Delta S\text{ 0; }\Delta H\text{ 0}$(D) $\Delta \text{G 0; }\Delta S\text{ 0; }\Delta H\text{ 0}$

Last updated date: 19th Sep 2024
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Hint: Adsorption is considered to be an exothermic process which is explained theoretically and verified experimentally. As the particles come closer, the randomness in general decreases. Adsorption process is a feasible process at all temperatures.

As suggested in the hint, adsorption process released heat which means that change in enthalpy is always negative i.e. $\Delta H\text{ 0}$.
Due to adhesion during adsorption, the randomness of the molecules is reduced resulting in decrease in entropy. Hence change is entropy is negative i.e. $\Delta S\text{ 0}$.
$\Delta G\text{ = }\Delta H\text{ - }T\Delta S$
Hence change in Gibbs free energy($\Delta \text{G}$) is negative i.e. $\Delta \text{G 0}$.