Which of the following statements is correct | vedclass

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(B) $1$. Adsorption is a spontaneous process, so the Gibbs free energy change $\Delta G$ must be negative $(\Delta G < 0)$.$2$. The relationship is gi

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$\Delta S$ is negative and therefore, $\Delta H$ should be highly negative.

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(B) $1$. Adsorption is a spontaneous process, so the Gibbs free energy change $\Delta G$ must be negative $(\Delta G $2$. The relationship is given by $\Delta G = \Delta H - T\Delta S$.$3$. During adsorption, gas molecules are trapped on the surface, leading to a decrease in randomness, so $\Delta S$ is negative.$4$. For $\Delta G$ to be negative when $\Delta S$ is negative, the term $\Delta H$ must be sufficiently negative to overcome the positive value of $-T\Delta S$ (since $-T\Delta S$ becomes positive).$5$. Thus, $\Delta H$ must be highly negative for the process to be spontaneous.

Which of the following statements is correct for the spontaneous adsorption of a gas on a solid surface?

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