To solve this problem, we need to understand the thermodynamics of adsorption.$\\$Adsorption is an exothermic process, meaning it releases heat. This implies that $\Delta H$ is negative.$\\$Let's analyze each option:$\\$Option 1: $\Delta G$ is negative, but $\Delta H$ and $\Delta S$ are positive.$\\$• For adsorption, $\Delta H$ should be negative, not positive. So, this option is incorrect.$\\$Option 2: $\Delta G, \Delta H$ and $\Delta S$ all are negative.$\\$• $\Delta G$ is negative because adsorption is a spontaneous process.$\\$• $\Delta H$ is negative because adsorption is exothermic.$\\$• $\Delta S$ is negative because the randomness decreases when molecules adhere to a surface.$\\$• This option correctly describes adsorption.$\\$Option 3: $\Delta G$ and $\Delta H$ are negative, but $\Delta S$ is positive.$\\$• $\Delta S$ should be negative, not positive, as the system becomes more ordered.$\\$• This option is incorrect.$\\$Option 4: $\Delta G$ and $\Delta S$ are negative, but $\Delta H$ is positive.$\\$• $\Delta H$ should be negative, not positive, as adsorption is exothermic.$\\$• This option is incorrect.$\\$Therefore, the correct option is Option 2, where $\Delta G, \Delta H$ and $\Delta S$ all are negative.