$$H=U+pV$$
Above is the formula for enthalpy or the sum of the internal energy and pressure volume product.
$-p\Delta V$ is work done by or on the system. But $pV$, yet very similar to work, I think, calculates the whole “cylinder”. Instead of just calculating the height difference of the cylinder before and after the air is condensed, it calculate the height of whole cylinder.
But anyway this is just my guess, what is it really?
Enthalpy $H$ is defined so that $\Delta H = q_P$, the heat at constant pressure. This is convenient for constant-pressure calorimetry---it makes it possible to track energy changes without considering volume changes in the system.
$$\begin{align*}\Delta U &= q + w & \text{(first law)}\\ \Delta U_P &= q_P + w_P & \text{(constant pressure)}\\ \Delta U_P &= \Delta H + w_P & \text{(definition of enthalpy)}\\ \end{align*}$$
...so the difference between $\Delta H$ and $\Delta U$ can be interpreted as minus the work for a constant pressure process.
But this doesn't answer your question for a general process. If the process is not constant pressure, we can still apply the definition of enthalpy, but the difference isn't minus the expansion work anymore. But what is it, then? How can we use something we've defined for a constant pressure process for all processes in general?
We'd like a new thermodynamic function $H$ that includes all of the information in $U$. We have $$dU = TdS - PdV$$ so the natural variables of $U$ are $S$ and $V$. We want this new function $H$ to have $P$ as a natural variable in place of $V$, so it will be convenient for constant-pressure calorimetry. Consider the following plot of $U$ vs. $V$:
The equation for the tangent line at some value of $V$ is $$ U = \left(\frac{\partial U}{\partial V}\right)_S V + intercept$$
If we define the new function as the intercept of the tangent line shown in the graph, it will have the properties we need:
$$H \equiv U - \left(\frac{\partial U}{\partial V}\right)_S V$$
You can see that the derivative $\left(\dfrac{\partial U}{\partial V}\right)_S = -P$ from the equation for $dU$ above. Then
$$H \equiv U - (-P) V = U + PV$$
so
$$dH = dU + d(PV) = TdS - PdV + PdV + VdP = TdS + VdP$$
By adding $PV$ to $U$, we've transformed the information in $U$ (with natural variables $S$ and $V$) to a new function $H$ (with natural variables $S$ and $P$).
This trick is called a Legendre transformation, and it can be used to understand the definitions of other thermodynamic functions like $G$ and $A$ as well.
The best thing I found was on wikipedia, I couldn't explain it in a better way:
The U term can be interpreted as the energy required to create the system, and the pV term as the energy that would be required to "make room" for the system if the pressure of the environment remained constant. When a system, for example, n moles of a gas of volume V at pressure p and temperature T, is created or brought to its present state from absolute zero, energy must be supplied equal to its internal energy U plus pV, where pV is the work done in pushing against the ambient (atmospheric) pressure.
