Pressure effects on chemical equilibria
For reactions where ēngas is not zero:
If the reaction volume is decreased (pressure increased), the reaction
shifts so that the total number of gas molecules decreases.
If the reaction volume is increased (pressure decreased), the reaction
shifts so that the total number of gas molecules increases.
For reactions where ēngas is zero, there are no volume/pressure
effects on the equilibrium position.
Like [ ], pressure changes do not alter K.
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