Which of the following is true with respect t | vedclass

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(B) For any spontaneous adsorption process,the Gibbs free energy change,$ \Delta G $,must be negative $( \Delta G < 0 )$. Adsorption is an exothermic

Vedclass · Accepted Answer

$ \Delta H < 0, \Delta S < 0, \Delta G < 0 $

Vedclass · Answer

(B) For any spontaneous adsorption process,the Gibbs free energy change,$ \Delta G $,must be negative $( \Delta G Adsorption is an exothermic process,meaning heat is released,so the enthalpy change,$ \Delta H $,is negative $( \Delta H Since gas molecules are restricted to the surface upon adsorption,the randomness of the system decreases,leading to a negative entropy change,$ \Delta S < 0 $.

Which of the following is true with respect to chemical adsorption?

Similar Questions

Adsorption is always

Assertion : The enthalpy of physisorption is greater than chemisorption.
Reason : Molecules of adsorbate and adsorbent are held by van der Waal's forces in physisorption and by chemical bonds in chemisorption.

Which of the following statements is correct for physisorption?

Give the differences between physical adsorption and chemical adsorption.

Assertion $(A)$: van der Waals' forces are responsible for chemisorption.
Reason $(R)$: High temperature is favourable for chemisorption.
The correct answer is

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