Endothermic vs exothermic

[504939134]

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.

[Connie Chen 1E]

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.

[DLee_1L]

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

[William Francis 2E]

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.

[Alice Chang 2H]

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