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Eileen Si 3G wrote:How does increasing or decreasing the partial pressure of a reactant affect the partial pressure of the product, and vice versa for a change in product and its effect on the reactant?
Think of equilibrium as an unbalanced see-saw where one side is supposed to have a different "weight" than the other, but it reaches a point of equilibrium where the ratio of R/P is ideal. Here's a short way to show what happens when partial pressures of reactants/products change.
Reactants increase -> Products favored
Reactants decrease -> reactants favored
Products decrease -> products favored
Products increase -> reactants favored
And it also may be worth noting that when dealing with changes in concentration of certain gases (pressures etc.), only increasing pressure by decreasing volume will have an effect on the concentration of the compound. If pressure is increased by adding an inert gas, as Professor Lavelle made note of, the concentration of the compound in Mol L^-1 does not change (n/v does not change).
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