Summary of Le Chatelier

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TanveerDhaliwal3G
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Joined: Fri Aug 30, 2019 12:17 am

Summary of Le Chatelier

Postby TanveerDhaliwal3G » Mon Jan 20, 2020 1:09 pm

What are all the components of Le Chatelier's Principle?

Tiffany_Chen 2K
Posts: 106
Joined: Fri Aug 30, 2019 12:15 am

Re: Summary of Le Chatelier

Postby Tiffany_Chen 2K » Mon Jan 20, 2020 1:32 pm

Chemical equilibriums will shift accordingly to minimize stressors. In lecture, we covered stressors such as concentration, pressure, and heat.

GFolk_1D
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Joined: Fri Aug 09, 2019 12:15 am

Re: Summary of Le Chatelier

Postby GFolk_1D » Mon Jan 20, 2020 4:28 pm

This is a great summary of the concept! https://www.khanacademy.org/science/che ... -principle

Ryan Lee 1E
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Joined: Sat Aug 17, 2019 12:16 am

Re: Summary of Le Chatelier

Postby Ryan Lee 1E » Mon Jan 20, 2020 10:05 pm

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.

Justin Quan 4I
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Re: Summary of Le Chatelier

Postby Justin Quan 4I » Tue Jan 21, 2020 10:23 am

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.

romina_4C
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Joined: Thu Jul 11, 2019 12:17 am

Re: Summary of Le Chatelier

Postby romina_4C » Tue Jan 21, 2020 11:32 am

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


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