For a gas in equilibrium with a liquid, the ratio of the concentration of the gas in the solution phase to that in the gaseous phase is constant at constant temperature, only if molecules undergo:

ionisation

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dissociation

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isolation

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reaction with solvent

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Solution

The correct option is A isolation
According to the Henry's law,
$\frac{(C o n c e n t r a t i o n o f g a s i n s o l u t i o n}{C o n c e n t r a t i o n o f g a s i n t h e g a s e o u s p h a s e)} = C o n s t a n t$
Only when there is simple solvation (isolation then stabilization). Not possible in the case of ionisation or dissociation.

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The active masses of pure solid or liquid phasesare not included in the expression of equilibrium constant as:
a)solid and liquid concentrations are independent of their quantities
b)solids and liquids react very slowly
c)solids and liquids at equilibrium do not interact with gaseous phase

d)the molecules of solids and liquids do not migrate to the gaseous phase

The active masses of pure solid or liquid phasesare not included in theexpression of equilibrium constant as:
a)solid and liquid concentrations are independent of their quantities
b)solids and liquids react very slowly
c)solids and liquids at equilibrium do not interact with gaseous phase

d)the molecules of solids and liquids do not migrate to the gaseous phase

Q. In the following gaseous phase equilibrium at constant temperature.