Why is the adsorption of a gas on a solid exo | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) Adsorption is a spontaneous process where gas molecules are trapped on the surface of a solid. According to the Gibbs free energy equation,$\Delta

Vedclass · Accepted Answer

Decrease in entropy.

Vedclass · Answer

(A) Adsorption is a spontaneous process where gas molecules are trapped on the surface of a solid. According to the Gibbs free energy equation,$\Delta G = \Delta H - T\Delta S$. For a spontaneous process,$\Delta G$ must be negative. During adsorption,the freedom of movement of gas molecules decreases,leading to a decrease in entropy $(\Delta S Since $-T\Delta S$ becomes positive,for $\Delta G$ to be negative,the enthalpy change $(\Delta H)$ must be negative (exothermic).

Why is the adsorption of a gas on a solid exothermic?

Similar Questions

Which gas will be adsorbed on a solid to a greater extent?

Which of the following compounds is formed when tungsten adsorbs oxygen gas?

Which one of the following equations represents the Freundlich adsorption isotherm?

The surface area of $1 \, g$ of activated charcoal is $1000 \, m^2$. Assuming complete coverage and unimolecular adsorption,if the radius of an ammonia molecule is $10^{-8} \, cm$,then the volume of ammonia adsorbed at $STP$ on $44/7 \, g$ of carbon will be ........ $L$. $(N_A = 6 \times 10^{23})$

Vedclass Test Series

Exam Paper Generator

Online Exam Module