(D) $ \text{Physisorption} $ is an exothermic process,meaning the enthalpy of adsorption $( \Delta H_{\text{adsorption}} )$ is negative $( -Ve )$.It i

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$ \Delta H_{\text{adsorption}} $ is low and $ +Ve $.

(D) $ \text{Physisorption} $ is an exothermic process,meaning the enthalpy of adsorption $( \Delta H_{\text{adsorption}} )$ is negative $( -Ve )$.It involves weak $ \text{van der Waals} $ forces,resulting in a low enthalpy change,typically in the range of $ 20-40 \ kJ \ mol^{-1} $.Since it is an exothermic process,the correct statement is that $ \Delta H_{\text{adsorption}} $ is low and negative $( -Ve )$,making option $ D $ the incorrect statement.

Class 12 Chemistry Surface Chemistry Adsorption and Adsorption isotherm

Easy

Which of the following statements is incorrect w.r.t. $ \text{Physisorption} $?

KCET 2016 All KCET

A
The forces involved are $ \text{van der Waal's} $ forces.
B
More easily liquifiable gases are adsorbed easily.
C
Under high pressure it results into $ \text{Multi-molecular} $ layer on adsorbent surface.
D
$ \Delta H_{\text{adsorption}} $ is low and $ +Ve $.