How could you dissociate a diatomic molecule, at equilibrium, without changing the temperature of the system?...

How could you dissociate a diatomic molecule, at equilibrium, without changing the temperature of the system? [Suggested key words: equilibrium constant, concentration, ratio, volume...]

This is a P-Chem problem

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Expert Solution

Consider a diatomic molecule AB with dissociates into A+ and B- ions. Given that this reaction is at equilibrium. at equilibrium, concentration of AB and A+ and B- ions remains unchanged.

Dissociation of AB can be brought about be either increasing the concentration of AB or by decreasing the concentration of A+ and B- ions.

When A+ and B- ions are removed form reaction flask, the concentration of ions will decrease and concentration of AB will be more. Thus the system will be no longer in equilibrium. Equilibrium constant changes and the forward reaction is favoured. Thus dissociation of AB occurs.

When the concentration of AB is made to increase by adding diatomic molecule to the reaction system, AB concentration increases which results in the change in the equilibrium constant and dissociation of diatomic molecule is favoured..

Both of these can be done without changing the temperature of the system

queen_honey_blossom answered 1 year ago

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