Enthalpy is defined as follows

H = E + PV

Enthalpy is the sum of the internal energy
and pressure times volume.

We cannot measure the enthalpy of a system, but we can look at changes in enthalpy.

dH = dE + dPdV

to make life easier we will make certain that Pressure is held constant...

dH = dE + PdV

So, the change in enthalpy, dH, is equal to the change in internal energy, dE, plus PV work, PdV.

The expression for dH can be simplified.

dE = q + w

and work is - PdV

dE = qp - PdV

q is given the subscript "p" because
we are holding the pressure constant.

Substituting for dE in dH = dE + PdV gives

dH = qp - PdV + PdV

So, at constant pressure allowing for only PV work (no other kind of work occurring)

dH = qp


Enthalpy was defined so that we can talk about the amount of heat released or absorbed by a reaction when any work being done is PV work occuring at constant pressure.

DH < 0 then qp is negative which means heat is leaving the system. A process which releases heat is exothermic.

DH > 0 then qp is positive which means heat is being absorbed by the system. A process which absorbs heat is endothermic.

Remember this does not represent the change in the total energy content (internal energy, E) it just tells us how much heat energy is released during a change occuring under very specific conditions.