Final answer:
The change in internal energy for the process H₂O(l) → H₂(g) + 1/2 O₂(g) is equal to the change in enthalpy (∆H⁰) which is -285.8 kJ/mol.
Step-by-step explanation:
The change in internal energy for a process can be calculated using the equation:
ΔE = ΔH - PΔV
Where ΔE is the change in internal energy, ΔH is the change in enthalpy, P is the pressure, and ΔV is the change in volume. In this case, the equation H₂O(l) → H₂(g) + 1/2 O₂(g) represents the change in enthalpy for the reaction, which is -285.8 kJ/mol. Since the reaction involves a change in state from liquid to gas, we can assume that the change in volume is equal to zero. Therefore, the change in internal energy (∆E⁰) for the process would be equal to the change in enthalpy (∆H⁰).