Summary of Le Chatelier
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Re: Summary of Le Chatelier
Chemical equilibriums will shift accordingly to minimize stressors. In lecture, we covered stressors such as concentration, pressure, and heat.
Re: Summary of Le Chatelier
This is a great summary of the concept! https://www.khanacademy.org/science/che ... -principle
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Re: Summary of Le Chatelier
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.
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Re: Summary of Le Chatelier
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
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
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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