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This post covers equilibrium position changes resulting from changes in pressure. This applies when both reactants and products are in the gas state. Basically, increasing pressure causes gas-state equilibria to shift toward the side with fewer molecules. This happens in an attempt to return the equilibrium system to its original pressure. The idea is that the equilibrium side with fewer molecules is least affected by the increased pressure because that side has the lower partial pressure to begin with. Therefore the side with the lower partial pressure experiences a pressure increase when the equilibrium shifts toward that side. At the same time the other equilibrium side experiences a decrease in partial pressure as the equilibrium shifts away from it. In general, an increase in pressure will shift the equilibrium in the direction which produces the fewest number of molecules and a decrease in pressure will shift the equilibrium toward the side which results in the formation of more total gas molecules. The diagram below demonstrates the pressure-changing effect.
From the diagram, notice that the total number of molecules reduces as the equilibrium position shifts right at a higher pressure. Notice, also, that even though the higher pressure right-shifted equilibrium equation is not stoichiometrically correct, the shift is allowed to happen because the total atom-number of each element does not change!
That's all for this post! Have a good one!
A publication of http://www.excellenceinlearning.biz
This post covers equilibrium position changes resulting from changes in pressure. This applies when both reactants and products are in the gas state. Basically, increasing pressure causes gas-state equilibria to shift toward the side with fewer molecules. This happens in an attempt to return the equilibrium system to its original pressure. The idea is that the equilibrium side with fewer molecules is least affected by the increased pressure because that side has the lower partial pressure to begin with. Therefore the side with the lower partial pressure experiences a pressure increase when the equilibrium shifts toward that side. At the same time the other equilibrium side experiences a decrease in partial pressure as the equilibrium shifts away from it. In general, an increase in pressure will shift the equilibrium in the direction which produces the fewest number of molecules and a decrease in pressure will shift the equilibrium toward the side which results in the formation of more total gas molecules. The diagram below demonstrates the pressure-changing effect.
From the diagram, notice that the total number of molecules reduces as the equilibrium position shifts right at a higher pressure. Notice, also, that even though the higher pressure right-shifted equilibrium equation is not stoichiometrically correct, the shift is allowed to happen because the total atom-number of each element does not change!
That's all for this post! Have a good one!
A publication of http://www.excellenceinlearning.biz
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