Semc
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Hey guys, I was wondering if anyone could possibly help me out in understanding le Chatelier's principle in relation to equilibrium changes for temperature, concentration and pressure using equations. I'm with AQA doing AS chemistry btw


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jamez870
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I'm also on this course, what do you need help with specifically?
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Abbieastoria
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Basically Le chateliers principle says that whatever changes is applied to the equation the equilibrium will shift to counteract this change and restore order to the reaction.

so if temp increases equilibrium will shift to the direction that has an endothermic reaction.

if concentration of a substance increases equilibrium will shift to reduce this concentration.

if pressure increases the equilibrium will shift to the side of the equation which has the least amount of moles


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Frank the Tankk
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Well, a reaction in equilibrium will work against your change by shifting the position of equilibrium.

So, say you have a reversible reaction A + B = C + D and the forward reaction is exothermic (and thus the reverse being endothermic).

if you increase the temperature of the reaction you will create more A + B (as the reverse is endothermic) and so the reaction moves to achieve equilibrium byreleasing more energy in the forward reaction to reduce the temperature (and this reducing your change). Therefore, the position of equilibrium has shifted left by creating a change on the right.
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Scorlibran
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(Original post by Semc)
Hey guys, I was wondering if anyone could possibly help me out in understanding le Chatelier's principle in relation to equilibrium changes for temperature, concentration and pressure using equations. I'm with AQA doing AS chemistry btw


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Here is a good explanation http://www.chemguide.co.uk/physical/...hange.html#top, if you need any extra help just ask.
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Semc
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Thank you so much guys!


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