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Le chateliers principle

Posted: Fri Dec 08, 2017 10:42 pm
by Lorie Seuylemezian-2K
Can someone please explain this principle to me and how we are supposed to apply it?

Re: Le chateliers principle

Posted: Fri Dec 08, 2017 10:50 pm
by An Dang 3F
Le Chatliers' Principle is the idea that a chemical reaction will adjust to minimize the effects of change back to the equilibrium constant. For example, if one increases the pressure of the reaction then the volume will decrease and the reaction will move in the direction where there are fewer moles. If one decreases the pressure, then the volume will increase, and the reaction will proceed to the side where there are more moles. There is an exception because if we add an inert gas to the reaction it will increase the pressure, but it will not change the volume, so the concentrations of the reaction do not change.

Re: Le chateliers principle

Posted: Fri Dec 08, 2017 10:51 pm
by Emily Glaser 1F
This principles describes what happens when an equilibrium is affected and how it will achieve equilibrium again.

A(g) + B(g) <--> C(g) + D(g)

If I add more A, that means the system will favor the PRODUCTS, meaning it will make more products to adjust to the increase on the reactants side. B will decrease a little as well because A is using more of it up to produce more products.

Re: Le chateliers principle

Posted: Fri Dec 08, 2017 11:06 pm
by Rachel Wang
le Chatelier's principle is the idea that if a restraint is applied, the equilibrium will shift so as to counteract the effect of the restraint.
Adding products will shift the rxn left; adding reactants will shift the rxn right.
Adding pressure (decreasing volume) will shift rxn to side with less gas molecules; decreasing pressure (increasing volume) will shift rxn to side with more gas molecules.
Adding a catalyst won't affect equilibrium.
If endothermic, adding heat will shift rxn right. If exothermic, adding heat will shift rxn left.