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Postby Casandra » Fri Jan 18, 2019 7:22 pm

How does a change in pressure affect the equilibrium in a reaction?

Vincent Li 4L
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Re: Pressure

Postby Vincent Li 4L » Fri Jan 18, 2019 7:33 pm

In terms of the equilibrium constant, the value of K does not change unless temperature is affected. If the source of the pressure is caused by a change in volume, then the concentrations of the reactants and products change, which may cause either the forward or reverse reaction to be favored to return to equilibrium (the direction can be found by calculating Q and comparing it to K). If there is a change in pressure by the addition of an inert (noble) gas, then there is no effect on the equilibrium. This is because though it affects the pressure similar to volume changes, the concentrations of all the constituent gases do not change.

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Re: Pressure

Postby pamcoronel1H » Fri Jan 18, 2019 7:40 pm

If you increase the pressure, the reaction will favor the side with the fewer moles because since the volume available now is decreased, the reaction will want to take up the least space possible.

For example, in:

2 O3 --> 3 O2

If you increase the pressure here, the reaction will tend to favor the reactants since it has less moles on the reactant side than the product (2<3).

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Re: Pressure

Postby Rami_Z_AbuQubo_2K » Sat Jan 19, 2019 12:45 am

-If the pressure increases, the side with less concentration/mols will be favored.
-If the pressure decreases, the side with more concentration/mols will be favored.

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