Can someone please explain why :
1. If a reaction requires Heat, (is endothermic) while forming products, then heating will favor P (product) formation when additional heat is used.
2. If a reaction gives off heat, (is exothermic) while forming products, then heating will favor R formation when additional heat is used.
Thank you.
Endothermic vs exothermic
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Re: Endothermic vs exothermic
For endothermic reactions, since there is more heat, it will be easier to overcome the activation energy, thus making it easier to form more products. As a result, the products will be favored.
For exothermic reactions, the reverse reaction (P-->R) will be endothermic. So using the logic that the reverse reaction is endothermic, there will be more reactants formed, as it is the products of the reverse reaction.
For exothermic reactions, the reverse reaction (P-->R) will be endothermic. So using the logic that the reverse reaction is endothermic, there will be more reactants formed, as it is the products of the reverse reaction.
Re: Endothermic vs exothermic
If it helps, I always look at heat as if it is another substance in the chemical equation when given a le Chatlier question. This makes it easier to see whether a heat increase or decrease will lead to a shift to products or reactants
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Re: Endothermic vs exothermic
Endothermic reactions are hungry for heat. You can think of heat as a reactant in the equation necessary for the reaction to run: AB + heat <--> A + B. Therefore, when the reaction gets heat, it favors the forward reaction, resulting in a raised concentration of the products. The opposite is true for exothermic reactions; heat is a reactant for the reverse reaction so the reactants are favored when heat is added.
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Re: Endothermic vs exothermic
If you're more of a visual learner, Khan Academy has a video explaining Le Chatelier's Principle here: https://www.khanacademy.org/science/chemistry/chemical-equilibrium/factors-that-affect-chemical-equilibrium/v/le-chatelier-s-principle
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