Le Chatelier's Principle
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- Опубліковано 14 лип 2024
- 066 - Le Chatelier's Principle
In this video Paul Andersen explains how Le Chatelier's Principle can be used to predict the effect of disturbances to equilibrium. When a reversible reaction is at equilibrium disturbances (in concentration, temperature, pressure, etc.) will be offset to reach a new equilibrium. For examples when more reactants are added the reaction will move to the right to reestablish the equilibrium constant.
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Artist: Herman Jolly
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All of the images are licensed under creative commons and public domain licensing:
Eframgoldberg. English: An Overlay of the Same 99.9% Pure NO2/N2O4 Sealed in an Ampoule. From Left to Right -196C, 0C, 23C, 35C, 50C, July 16, 2013. Own work. commons.wikimedia.org/wiki/Fil....
en:User:Greenhorn1. English: Nitrogen Dioxide (NO2) on the Left and Dinitrogen Tetroxide (N2O4) on the Right., February 25, 2008. en:Image:N02-N2O4.jpg. commons.wikimedia.org/wiki/Fil....
"File:Ammonia-3D-vdW.png." Wikipedia, the Free Encyclopedia. Accessed January 3, 2014. en.wikipedia.org/wiki/File:Amm....
"File:Dinitrogen-Tetroxide-3D-vdW.png." Wikipedia, the Free Encyclopedia. Accessed January 3, 2014. en.wikipedia.org/wiki/File:Din....
"File:Tetrachlorocobaltate Aqueous Ion.jpg." Wikipedia, the Free Encyclopedia. Accessed January 3, 2014. en.wikipedia.org/wiki/File:Tet....
yinch. English: SVG Version of Nitrogen Molecule., November 25, 2010. Produced in Inkscape. commons.wikimedia.org/wiki/Fil....
mr Anderson we are indebted to you
I love your style of teaching. Soo much better than my chem teacher, who introduces something to us, barely explains, and expects us to be able to take a quiz on it the next day. >.>
Sounds like a lot of teachers... Very few like this guy!
Sandra Gonzalez lol, my teacher doesn't know how to teach either, to top it off we have a quiz on the same day he teaches us a new topic...
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mine does the same but then refuses to answer questions on it or go through it again come exams.
Our*, not "Are". What english class do you have by the way?
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3:17 am march 18, 2021 mid pandemic. Hello to the future students reading this comment. Its hard but youll learn it like he did and I did. Anyways tryna imagine life post pandemic wonder what that will be like. Anyways future student gotta go
Back go studying
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We’re deeply grateful for your help
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This goes hand in hand with the fact that when enthalpy is endothermic (delta H is greater than 0), then when it has a lot of temp it’s spontaneous (goes to the right) and when it lowers temp, it goes to the left is non spontaneous.
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let me know if you are okay with that!
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Btw, I also like your process of teaching: very straight forward, yet simple enough to apply and follow along :).
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simple and straight foward. i only know of the temp and pressure part. knowing the concentration helps also.
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In any reaction where it is reversible and we have reactant and products and equilibrium is reached, if there is ever a stress factor involved like increase/ decrease temperature, increase/ decrease pressure there is going to be a new equilibrium will be established. Increasing yield by concentration when we want more product we raise the concentration of the reactants to shift reaction towards the right and vice versa.
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Hey Great video however, with the reaction of N2O4 to 2NO2 when you increase pressure or decrease volume why would the reaction shift right first and then go to the side of fewer moles? I thought that it would shift left to reactants first and stay there till the volume would allow the product of nitrogen dioxide to form? A little confused
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Is the value of K in the new equilibrium going to be the same for the same temperature, or will there be a new K value?
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When more of a reactant or is added, will the new equilibrium have a different Kc (equilibrium constant) than our original reaction? Or will it remain constant?
Kc depends on Temperature
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Could you add examples of application that would have been helpful. Thanks
After we place a stress on the reaction (by removing/adding reactants) and allowing that reaction to come to a new equilibrium, does the new equilibrium still have the same equilibrium constant? Afterall, it is referring to the same chemical equation.
Yes, since for a given reaction, at a temperature, Kc stays the same. The only thing that changes is Q. When the equilibrium is thrown off, the value of Q will change (in other words, Q no longer equals to Kc). According to Le Chatelier's principle, the reaction will shift in the direction that restore the equation: Q = Kc.
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