Enthalieänderung

Enthalieänderung, often referred to as enthalpy change, is a fundamental concept in thermodynamics that quantifies the total heat content of a system. It is denoted by the symbol ΔH and represents the difference in enthalpy between the final state and the initial state of a system during a process. Enthalpy itself is a state function, meaning it depends only on the current condition of the system and not on the path taken to reach that condition.

In chemical reactions, the enthalpy change specifically refers to the heat absorbed or released during the reaction at constant pressure. If ΔH is negative, the reaction is exothermic, releasing heat into the surroundings. If ΔH is positive, the reaction is endothermic, absorbing heat from the surroundings. This measurement is crucial for understanding the energy balance of chemical transformations and is typically expressed in units of kilojoules per mole (kJ/mol) or joules per mole (J/mol). The enthalpy change can be experimentally determined through calorimetry or calculated using standard enthalpies of formation. Understanding enthalpy change allows for predictions about the feasibility and energy requirements of various processes.