# Le chateliers principle

(Difference between revisions)
 Revision as of 13:26, 6 December 2018 (view source) (Created page with " Le Chatelier's Principle states that an equilibrium's position will shift to counteract any constraints put upon it.") Revision as of 14:29, 6 December 2018 (view source) (I have updated the page showing how you can use Le Chatelier's principle to predict the outcome of applying different constraints to a reaction)Newer edit → Line 1: Line 1: −  Le Chatelier's Principle states that an equilibrium's position will shift to counteract any constraints put upon it. +  Le Chatelier's Principle states that an equilibrium's position will shift to counteract any constraints put upon it. + + This principle can be used to predict the outcome of applying a change in condition to a reaction for example: + + Increasing Temperature: + + For a reaction [P] ⇌ [R] + + If the forward reaction is [https://teaching.ncl.ac.uk/bms/wiki/index.php/Exothermic_reaction exothermic] it releases energy as products are formed. Increasing temperature will cause the equilibrium position to shift to the left to counteract this change and remove the increase in temperature from the system by taking in energy [P] -> [R]. + + Increasing Pressure: + + For a reaction [P](g) ⇌ 2[R](g) + + The forward reaction increases pressure as there are a greater number of gaseous moles on the RHS (right-hand side) of the equilibrium. Therefore, if the pressure of the system increases the equilibrium position will shift to the left to counteract the change (reduce system pressure)

## Revision as of 14:29, 6 December 2018

Le Chatelier's Principle states that an equilibrium's position will shift to counteract any constraints put upon it.

This principle can be used to predict the outcome of applying a change in condition to a reaction for example:

Increasing Temperature:

For a reaction [P] ⇌ [R]

If the forward reaction is exothermic it releases energy as products are formed. Increasing temperature will cause the equilibrium position to shift to the left to counteract this change and remove the increase in temperature from the system by taking in energy [P] -> [R].

Increasing Pressure:

For a reaction [P](g) ⇌ 2[R](g)

The forward reaction increases pressure as there are a greater number of gaseous moles on the RHS (right-hand side) of the equilibrium. Therefore, if the pressure of the system increases the equilibrium position will shift to the left to counteract the change (reduce system pressure)