Which of the following statements is false du | vedclass

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(A) Adsorption is a spontaneous process, which implies that the Gibbs free energy change $(\Delta G)$ must be negative $(\Delta G < 0)$.
Since gas

Vedclass · Accepted Answer

Enthalpy change is positive

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(A) Adsorption is a spontaneous process, which implies that the Gibbs free energy change $(\Delta G)$ must be negative $(\Delta G < 0)$.
Since gas molecules are adsorbed onto a solid surface, their freedom of movement decreases, leading to a decrease in entropy $(\Delta S < 0)$.
From the equation $\Delta G = \Delta H - T\Delta S$, for $\Delta G$ to be negative when $\Delta S$ is negative, the enthalpy change $(\Delta H)$ must be negative $(\Delta H < 0)$.
Therefore, adsorption is an exothermic process, meaning heat is released, and the enthalpy change is negative.
Thus, the statement that 'Enthalpy change is positive' is false.

Which of the following statements is false during the adsorption of gas molecules on a metal surface?

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