Question
Adsorption of a gas on the surface of solid is generally accompanied by a decrease in entropy still it is a spontaneous process. Why?
✓
Answer
According to the equation:
$\Delta\text{G}=\Delta\text{H}-\text{T}\Delta\text{S}$
For a process to be spontaneous, $\Delta\text{G}$ should be negative. Even though ΔS is negative here, $\Delta\text{G}$ is negative because reaction is highly exothermic, i.e., $\Delta\text{H}$ is negative.
$\Delta\text{G}=\Delta\text{H}-\text{T}\Delta\text{S}$
For a process to be spontaneous, $\Delta\text{G}$ should be negative. Even though ΔS is negative here, $\Delta\text{G}$ is negative because reaction is highly exothermic, i.e., $\Delta\text{H}$ is negative.
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