Change in Enthalpy in Free Expansion of Ideal and Real gas against Vacuum By free expansion, I am referring to gas allowed to expand freely against vacuum in a Joule Expansion.
If gas is ideal then change in Internal Energy '∆U' and change in Enthalpy '∆H' is zero.
(By ∆H = ∆U + nR∆T).
But I was wondering whether '∆H' would still be zero for real gas?
(I know that ∆U will be zero for real gas. I just want to ask about ∆H)
In the Joule experiment, $\Delta H$ is not zero for a real gas.  $\Delta H=\Delta U+\Delta (PV)$, and even if $\Delta U$ is zero, there is no physical reason to expect that $\Delta (PV)$ would be zero in this process.