Our learning objectives for Feb. 7 are to be able to:
- explain Le Chatelier’s principle;
- identify potential disturbances to a system at equilibrium; and
- predict, using Le Chatelier’s principle, the effect of a disturbance on a chemical equilibrium.
Before class on Feb. 7:
- please watch the video below (22 min.)
- complete the notes
- and make a comment.
https://www.youtube.com/watch?v=laawq0LkZZc
chemistry matters 
In this video I learned about Le Chatelier’s Principle and how changing different elements such as temperature, pressure, and concentration affect equilibrium position. A disturbance in the force will be counteracted. If more concentration of reactant is added, the system will shift right. If more concentration of product is added, it will shift left. If the volume is decreased(pressure increased), then the system will shift in the direction of the least moles of gas, if the volume is increased(pressure decreased), the system will shift in the direction of the most moles of gas. When a reaction is exothermic and heat is added, the system shifts left. In an exothermic reaction, heat would be considered a product, so the system will shift to make more reactant. If a reaction is endothermic, then the reaction shifts to the right to make more products. In this instance, heat is considered a reactant. Catalysts do not have an effect on equilibrium composition.
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I learned about what Le Chatelier’s principle is and how that affects the way the equilibrium in a reaction shifts. If there’s a disturbance in the force, the system will shift in the opposite direction.
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Today I learned how to determine which way a chemical reaction must balance in order to reach new equilibrium if it is thrown off. Temperature, pressure, and Adding or diminishing a reactant or a product can determine which way the reaction needs to go to counterbalance the effects. Adding a catalyst, however, only lowers the activation energy of the entire reaction, therefore allowing it to maintain equilibrium.
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In this video, I learned about the Le Chatelier’s Principle regarding the effects of changing temperature, pressure, or concentration on the equilibrium position. I also learned that catalysts do not affect the equilibrium position because it is the same for both the forward and reverse reaction.
Questions:
Wouldn’t increasing temperature in an endothermic reaction decrease K and increasing temperature in an exothermic reaction increase K instead?
Also, if the reaction is already at equilibrium, and the pressure is changed, wouldn’t the reaction change the same way for both reactants and products since they were in equilibrium (they are balanced) in the beginning and therefore would not change the equilibrium position? Or is it because of the exponents that the change in pressure, aka concentration, that makes the equilibrium position change?
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