If the enthalpy change for a reaction is given as -50 kJ, what type of reaction is this?

The enthalpy change of a reaction, indicated as -50 kJ, signifies that energy is released during the reaction. In thermodynamics, reactions that release heat to their surroundings are termed exothermic. When the enthalpy change is negative, it indicates that the products of the reaction have lower enthalpy compared to the reactants, demonstrating that energy has been released as a result of the reaction.

In contrast, an endothermic reaction absorbs energy from the surroundings, resulting in a positive enthalpy change. Equilibrium and reversible reactions pertain to the dynamic state of reactants and products in a reaction but do not specifically indicate the heat exchange involved. Thus, given the negative enthalpy change of -50 kJ, the reaction identified here is definitively exothermic, as it reflects a release of energy, confirming the correctness of identifying it as an exothermic reaction.