What is the difference between endothermic and exothermic reactions in equilibrium?

Endothermic reactions absorb heat, while exothermic reactions release heat, affecting the position of equilibrium differently.

In an endothermic reaction, heat is absorbed from the surroundings, causing the reaction to feel cold. This is because the energy required to break the bonds in the reactants is greater than the energy released when new bonds are formed in the products. In terms of equilibrium, if you increase the temperature, the equilibrium position will shift to the right, favouring the endothermic reaction to absorb the extra heat. Conversely, if you decrease the temperature, the equilibrium will shift to the left, favouring the exothermic reaction.

On the other hand, exothermic reactions release heat into the surroundings, making the reaction feel hot. This is because the energy released when new bonds are formed in the products is greater than the energy required to break the bonds in the reactants. In terms of equilibrium, if you increase the temperature, the equilibrium position will shift to the left, favouring the endothermic reaction to absorb the extra heat. Conversely, if you decrease the temperature, the equilibrium will shift to the right, favouring the exothermic reaction.

In summary, the direction of an equilibrium shift due to a change in temperature depends on whether the reaction is endothermic or exothermic. This is based on Le Chatelier's principle, which states that a system in equilibrium will adjust to counteract any change imposed on it. Therefore, understanding the difference between endothermic and exothermic reactions is crucial for predicting how changes in temperature will affect a reaction in equilibrium.