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The term exothermic is used to denote reactions that release energy in the form of heat when they are carried out. Conversely, endothermic denotes reactions that require energy (which they acquire by absorbing heat from surroundings) to be carried out.
You need to know this for the test too. Adding heat changes the Q value for a reaction. If a reaction is endothermic that means heat is on the left side (reactants side) of the equation, while exothermic reactions have heat being released on the products side. You treat heat as a reactant or product and decipher the effect it will have on Q value.
Le Chatelier's Principle refers to the process of chemical reactions adjusting to minimize the affect of certain changes. Moreover, exothermic means that heat is released as a part of the reaction and endothermic means that heat is required for the reaction to proceed.
An endothermic reaction is when delta H is positive and energy is absorbed, so the surroundings cool. An exothermic reaction is when delta H is negative and energy is released, so the surroundings are warm. Applying Le Chatelier's principle, if heat is added to an endothermic reaction, the reaction would shift right and favor the products. If heat is added to an exothermic reaction, the reaction would shift left and favor the reactants.
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