Le Chatelier's Principle

Moderators: Chem_Mod, Chem_Admin

Karyn Nguyen 1K
Posts: 72
Joined: Fri Apr 06, 2018 11:04 am

Le Chatelier's Principle

Postby Karyn Nguyen 1K » Sun Jan 20, 2019 4:45 pm

Can someone explain why changing the concentration doesn't change K but changing the temperature does?

Karyn Nguyen 1K
Posts: 72
Joined: Fri Apr 06, 2018 11:04 am

Re: Le Chatelier's Principle

Postby Karyn Nguyen 1K » Sun Jan 20, 2019 4:47 pm

Also, since Le Chatelier's principle is only used at equilibrium what do we use if it's not at equilibrium?

Porus_Karwa_2E
Posts: 72
Joined: Fri Sep 28, 2018 12:24 am

Re: Le Chatelier's Principle

Postby Porus_Karwa_2E » Sun Jan 20, 2019 4:57 pm

Changing the concentration doesn't change K because if we take out more reactants the equation will shift in order to make up for the deficient amount of reactants to make the K ratio the same.

caseygilles 1E
Posts: 73
Joined: Fri Sep 28, 2018 12:18 am

Re: Le Chatelier's Principle

Postby caseygilles 1E » Sun Jan 20, 2019 5:20 pm

Changing the concentration doesn't change K because the system will settle back to the same ratio of K even if the concentrations are different. The system looks to minimize the effect of changes so when equilibrium is perturbed it slowly settles back to its stable equilibrium ratio. For instance, if we take out some product, the the reaction ill shift right to form more of that product and the same equilibrium constant ratio of products over reactants will return.
Changing the temperature changes K because it depends on whether the reaction is endothermic or exothermic. Essentially, raising the temperature of a reaction mixture at equilibrium will shift the reaction in the endothermic direction. K changes depending on whether product or reactant is favored due to temperature changes.


Return to “Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions”

Who is online

Users browsing this forum: No registered users and 1 guest