What Changes The Equilibrium Constant In An Equilibrium System, And Why?
April 27th, 2009
Why does increasing the temperature change the equilibruim constant?
Why don’t:
-adding more of a reactant, (or product?)
-increasing pressure, (more generally, changing the pressure?)
-adding a catalyst
change the equilibrium constant?
(If this info is wrong or something, then please correct me). 
Entry Filed under: Equilibrium Chemistry
2 Comments Add your own
1. spidey | April 27th, 2009 at 11:00 pm
There’s NOTHING that can be able to change equilibrum constant except TEMPRETURE.
-Adding more catalyst speeds up rate of equilibrum reaching but the equilibrium constant stays the same.
-Increasing Pressure doesn’t change the constant, it justs shifts the equlibrium towards less number of moles but the ratio between them stays the same.
-Adding more reactants or products,shifts the reaction towards the opposite (i mean if reactants is added so more products is formed and vice versa), and ratio stays the same
Le Chatelier’s principle is applied when direction of equilibrium shifting is needed to be known not calculating Equilibrium constant.
The Equilibrum constant is a RATIO not a RATE between reactants and products according to thier molar ratios.
YOUR INFO IS TOTALLY CORRECT.
2. shaq | April 27th, 2009 at 11:00 pm
u should look for le chatelier rule
this link can help u:http://en.wikipedia.org/wiki/Le_Chatelie…
the other things u listed also change rate of forward or backward reactions so they also change the reaction rate constant yes ur info is wong
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