Why is there no impact of pressure on a equilibrium condition when the number of molecule of gas reactant and the number of molecule of gas product are same? What will the theoretical explanation?
1 Answer
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Let's take a sample gaseous equilibrium:
At equilibrium,
When pressure is changed, you might think that
This doesn't happen, however!
When the volume is changed to cause a change in pressure, yes, the concentration will change.
And, since there's an equal number of moles on each side, these changes will cancel out (since you can factor out a constant raised to
It's unaffected, so the system is still at equilibrium and the position does not change.