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## Homework Statement

I know that for constant volume ∂q=du and so du=Cv.dT

However i don't understand how did we get to ∂q=du by neglecting the vdP term of enthalpy

What I am trying to say is, is enthalpy this ∆U+P∂V+V∂P or this ∆U+P∂V? I don't 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

## Homework Equations

## The Attempt at a Solution

From what I see:

∂Qnet,in=∆U+∂Wnet,out

∂Qnet,in=∆U+P∂V+V∂P

C=∂Qnet,in/dT

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?