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Determining Equilibrium Reaction Direction

Posted: Mon Jan 06, 2020 1:10 pm
by Giselle Littleton 1F
When determining the direction of an equilibrium reaction, how do you know whether to use 10^3/10^-3 or 1 as a comparison to K? I've seen both 1 and 10^3/10^-3 being used.

Re: Determining Equilibrium Reaction Direction

Posted: Mon Jan 06, 2020 3:33 pm
by Sam McNeill 1E
I believe that the 10^3 is referencing acids and bases, as Dr. Lavelle mentions in the video module.

Re: Determining Equilibrium Reaction Direction

Posted: Mon Jan 06, 2020 3:45 pm
by Amy Pham 1D
Comparing K to 10^3 and 10^-3 will tell you which direction the reaction proceeds to. Values in between these numbers do not indicate any strong favoring toward products not reactants, but can still tell you which reaction (forward or reverse) is happening -slightly- more. If K<0, the reactants are slightly favored and if K>0 the products are slightly favored.

Re: Determining Equilibrium Reaction Direction

Posted: Mon Jan 06, 2020 7:27 pm
by WesleyWu_1C
To determine the direction of an equilibrium reaction you can just compare K to 1. If K <1, than the reaction favors the reactants and if K >1 then the reaction favors the products. Dr. Lavelle uses 10^3 or 10^-3 as comparison when he uses strongly favors. For example, if K<1, the reaction favors the reactants and if K < 10^-3, the reaction strongly favors the reactants. I hope this helps.