Which of the following statements is correct | vedclass

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(B) The spontaneity of a process is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T \Delta S$.For a process to be spontaneous,$

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

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(B) The spontaneity of a process is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T \Delta S$.For a process to be spontaneous,$\Delta G$ must be negative.During the adsorption of a gas on a solid surface,the gas molecules become restricted,leading to a decrease in randomness,so $\Delta S Substituting this into the equation: $\Delta G = \Delta H - T(	ext{negative}) = \Delta H + T \Delta S$.For $\Delta G$ to be negative,$\Delta H$ must be sufficiently negative to overcome the positive $T \Delta S$ term.Therefore,$\Delta H$ must be highly negative.

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

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