Which of the following parameters is text{cor | vedclass

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(B) Adsorption is a spontaneous process,so $\Delta G < 0$.It is an exothermic process,so the enthalpy change $\Delta H < 0$.Since gas molecules are ad

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$\Delta S_{	ext{surrounding}} > 0$

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(B) Adsorption is a spontaneous process,so $\Delta G It is an exothermic process,so the enthalpy change $\Delta H Since gas molecules are adsorbed on the solid surface,their freedom of movement decreases,leading to a decrease in entropy,so $\Delta S_{	ext{system}} For a spontaneous process,the total entropy change $\Delta S_{	ext{total}} = \Delta S_{	ext{system}} + \Delta S_{	ext{surrounding}} > 0$.Since $\Delta S_{	ext{system}}$ is negative,$\Delta S_{	ext{surrounding}}$ must be positive and greater in magnitude than $|\Delta S_{	ext{system}}|$ to make the process spontaneous. Thus,$\Delta S_{	ext{surrounding}} > 0$ is the correct parameter.

Which of the following parameters is $\text{correct}$ regarding the adsorption of gases over a solid?

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