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Summary of Le Chatelier

Posted: Mon Jan 20, 2020 1:09 pm
by TanveerDhaliwal3G
What are all the components of Le Chatelier's Principle?

Re: Summary of Le Chatelier

Posted: Mon Jan 20, 2020 1:32 pm
by Tiffany_Chen 2K
Chemical equilibriums will shift accordingly to minimize stressors. In lecture, we covered stressors such as concentration, pressure, and heat.

Re: Summary of Le Chatelier

Posted: Mon Jan 20, 2020 4:28 pm
by GFolk_1D
This is a great summary of the concept! https://www.khanacademy.org/science/che ... -principle

Re: Summary of Le Chatelier

Posted: Mon Jan 20, 2020 10:05 pm
by Ryan Lee 1E
In addition, note that K will only change with temperature, which means adding additional product/reactant or changing pressure does not change K. If product/reactant is added or pressure is changed, you can simply calculate Q and then find what way the reaction will proceed by comparing Q to K.

Re: Summary of Le Chatelier

Posted: Tue Jan 21, 2020 10:23 am
by Justin Quan 4I
To summarize, Le Chatelier's is a set of principles or guidelines that predicts the effect of a change to a system under equilibrium conditions. It basically states that when a system experiences a disturbance, it will respond to restore a new equilibrium state. Factors that would change equilibrium include changes in temperature, concentration, and partial pressure for gas reactions.

Re: Summary of Le Chatelier

Posted: Tue Jan 21, 2020 11:32 am
by romina_4C
Le Chatalier's principle states that, when put under stress, the reaction will shift in a way to minimize the stress.

For example
-adding reactants - reaction shifts to the right to form more products
-adding products - reaction shifts to the left to form more reactants
-removing reactants - reaction shifts to the left to form more reactants
-removing products - reaction shifts to the right to form more products
-increasing volume (decreasing pressure) - reaction shifts to side of equation with more moles of gas
-decreasing volume (increasing pressure) - reaction shifts to side of equation with fewer moles of gas
None of the above examples (changing pressure, concentration) change the value of the equilibrium constant. However, changing temperature does change the value of K.

For an endothermic reaction (where heat is a reactant)
-increasing temp - reaction shifts to right to form more products
-decreasing temp - reaction shifts to left to form more reactants

For an exothermic reaction (where heat is a product)
-increasing temp - reaction shifts to left to form more reactants
-decreasing temp - reaction shifts to right to form more products