Under what conditions would enthalpy be equal to the change in internal energy (ΔE)? Group of answer choiceswhen energy is conservedwhen no change in volume occurswhen pressure increases0 degrees C

Enthalpy (H) is equal to the change in internal energy (ΔE) when no work is done by or on the system, which typically occurs when there is no change in volume. This is because enthalpy is defined as H = E + PV, where E is the internal energy, P is the pressure, and V is the volume. The change in enthalpy (ΔH) is therefore ΔE + PΔV. If there is no change in volume (ΔV = 0), then the PΔV term drops out, and ΔH = ΔE. So, the correct answer is "when no change in volume occurs".

Enthalpy (H) is equal to the change in internal energy (ΔE) when no work is done by or on the system, meaning there is no change in volume. This is because enthalpy is defined as H = E + PV, where E is the internal energy, P is the pressure, and V is the volume. The change in enthalpy (ΔH) is therefore ΔE + PΔV. If there is no change in volume (ΔV = 0), then ΔH = ΔE. This is typically the case in processes that occur at constant pressure and do not involve gases, or in processes involving gases where the change in volume is negligible.