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Which of the following statements is incorrect w.r.t. Physisorption ?
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The correct answer is:
\( \Delta H_{\text {adsorption }} \) is low and \( +V e \)
Physisorption is an exothermic process but, its enthalpy ofadsorption is low, because attractive forces between
adsorbent and the adsorbate molecules are weak (i.e., van der Waals forces) and therefore, molar enthalpy ( \( \Delta \mathrm{H} \) ) of
adsorption is low and is of the order of \( 20-40 \mathrm{~kJ} \mathrm{~mol}^{-1} \). Maximum of gas is adsorbed when pressure is increased as
the volume of gas decreases. The gases which are easily liquefied are adsorbed readily, because van der Waals forces
are stronger near the critical temperature.
adsorbent and the adsorbate molecules are weak (i.e., van der Waals forces) and therefore, molar enthalpy ( \( \Delta \mathrm{H} \) ) of
adsorption is low and is of the order of \( 20-40 \mathrm{~kJ} \mathrm{~mol}^{-1} \). Maximum of gas is adsorbed when pressure is increased as
the volume of gas decreases. The gases which are easily liquefied are adsorbed readily, because van der Waals forces
are stronger near the critical temperature.
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