# Enthalpy vs Heat

If we have a closed cylinder filled with a gas and we heat it, by $$1^{st}$$ law we have: $$\Delta q=\Delta U$$ (?) since $$\Delta V$$ = 0. But $$\Delta H= \Delta U+ V. \Delta P$$.

What does that difference between the enthalpy change and heat supplied physically signify in this case?