# Le Chateliers principle and increase in temperature [duplicate]

If you increase the temperature, the endothermic reaction is favored. The Le Chatelier's principle states that the endothermic reaction is favored in order to minimize the effect of an increase in temperature. Endothermic reactions absorb heat so the temperature must, in a way, remain constant in that system. So that way, the equilibrium constant is never changed due to a change in temperature as the temperature doesn't change. I know I went wrong somewhere but can someone explain where. Please don't include equations like the ones with Gibbs free energy and Van't hoff equations and stuff as we didn't learn all of that in school yet. Please make the explanation as intuitive as possible.

• Are you confusing the reaction being endothermic or exothermic with the system being isothermal or adiabatic? – MaxW Feb 4 at 4:34
• You may perhaps have an idea endothermic reaction absorbs near all provided thermal energy. It is not like that, it absorbs just a small part. ...in order to minimize the effect... is misleading. "to decrease the effect" is more correct. – Poutnik Feb 4 at 8:16
• Heat is not a species in the reaction. It does not enter into the equilibrium expression. Therefore, you cannot apply Le Châtelier's Principle. – Zhe Feb 4 at 14:02