Answer: ΔH = H(final state) - H(initial state)
Step-by-step explanation:
he change in enthalpy of a system can be determined using the equation:
ΔH = H(final state) - H(initial state)
In this equation, ΔH represents the change in enthalpy, H(final state) represents the enthalpy of the system in the final state, and H(initial state) represents the enthalpy of the system in the initial state.
Enthalpy is a measure of the heat energy in a system, and the change in enthalpy represents the amount of heat energy gained or lost during a process. It can be positive if heat is absorbed by the system (endothermic process) or negative if heat is released by the system (exothermic process).
an example to better understand this equation. Imagine we have a chemical reaction where 2 moles of substance A react to form 3 moles of substance B. If we know the enthalpy of substance A in its initial state and the enthalpy of substance B in its final state, we can calculate the change in enthalpy.
For instance, if the enthalpy of substance A in its initial state is 50 kJ/mol and the enthalpy of substance B in its final state is 80 kJ/mol, we can calculate the change in enthalpy as follows:
ΔH = H(final state) - H(initial state)
ΔH = 80 kJ/mol - 50 kJ/mol
ΔH = 30 kJ/mol
Therefore, the change in enthalpy for this reaction is 30 kJ/mol. This means that the reaction is exothermic, as heat is released by the system.
In summary, the equation ΔH = H(final state) - H(initial state) can be used to determine the change in enthalpy of a system. It allows us to calculate the heat energy gained or lost during a process and helps us understand whether the process is endothermic or exothermic.