Answer

Adsorption is always exothermic. This statement can be explained in two ways.(i) Adsorption leads to a decrease in the residual forces on the surface of the adsorbent. This causes a decrease in the surface energy of the adsorbent. Therefore, adsorption is always exothermic.

(ii) ΔH of adsorption is always negative. When a gas is adsorbed on a solid surface, its movement is restricted leading to a decrease in the entropy of the gas i.e., ΔS is negative. Now for a process to be spontaneous, ΔG should be negative.ΔG = ΔH - TΔSSince ΔS is negative, ΔH has to be negative to make ΔG negative. Hence, adsorption is always exothermic.

This causes a decrease in the surface energy of the adsorbent. Therefore,adsorptionisalways exothermic. ... When a gas isadsorbedon a solid surface, its movement is restricted leading to a decrease in the entropy of the gas i.e., ΔS is negative. Now for a process to be spontaneous, ΔG should be negative.

Adsorption is always exothermic, this statement can be explained by two.i) Adsorption leads to a decrease in the residual forces on the surface of the adsorption.This cause a decrease in the surface energy of the adsorption therefore adsorption is always exothermic.ii)ΔH of adsorption is always negtive.When a gas is adsorbed on a soild surface its movement is restricted leading to decrease in the entropy of the gas i.e.ΔSAdsorption is accompanised by decrease in entropy, i.e., ΔS = – ve. If it is spontaneous then ΔG should be negative.ΔG = ΔH – TΔSSince ΔS is – ve, ΔG will be – ve only ifΔH = – ve, i.e., if process is exothermic.

This causes a decrease in the surface energy of the adsorbent. Therefore,adsorptionisalways exothermic. ... When a gas isadsorbedon a solid surface, its movement is restricted leading to a decrease in the entropy of the gas i.e., ΔS is negative. Now for a process to be spontaneous, ΔG should be negative.

This causes a decrease in the surface energy of the adsorbent. Therefore,adsorptionisalways exothermic. ... When a gas isadsorbedon a solid surface, its movement is restricted leading to a decrease in the entropy of the gas i.e., ΔS is negative. Now for a process to be spontaneous, ΔG should be negative.

Adsorption leads to a decrease in the residual forces on the surface of the adsorbent. This causes a decrease in the surface energy of the adsorbent. Therefore, adsorption is always exothermic.

(ii) ΔH of adsorption is always negative. When a gas is adsorbed on a solid surface, its movement is restricted leading to a decrease in the entropy of the gas i.e., ΔS is negative. Now for a process to be spontaneous, ΔG should be negative.

ΔG = ΔH - TΔS

Since ΔS is negative, ΔH has to be negative to make ΔG negative. Hence, adsorption is always exothermic.