I know that for constant volume ∂q=du and so du=Cv.dT
However i dont understand how did we get to ∂q=du by neglecting the vdP term of enthalpy
What im trying to say is, is enthalpy this ∆U+P∂V+V∂P or this ∆U+P∂V? I dont understand since the definition of enthalpy is derived out of a constant pressure volume change
And why snt specific heat at constant volume Cv=∆U+V∂P/dT instead of Cv=∆U/dT?
Thank you in advance for your answers
The Attempt at a Solution
From what I see:
For constant pressure:
Cp=∆U+P∂V/dT assuming ∆U+P∂V is enthalpy then ∆H=Cp.∆P
For constant volume:
Cv=∆U+V∂P/dT but all the books say it actually is just ∆U/dT
where did the VdP term go? if we add heat to a fixed volume won't its pressure increase and so VdP would be relevant?