Thermodynamics question

For
U = Cv*delta(T)
H = Cp*delta(T)

Since U, H, C and T are state properties, does this mean that both equations hold even when it is not a constant pressure/volume process?

In other words, do the two equations hold for ALL processes and fluids, or do they only hold for reversible and/or ideal gases processes? Thanks.

you derived this using the fundamental therodynamic relation, which is only applicaple if the work is reversible.

Cold = contract
Hot = expand

any questions?

>>3
counterexample: water at 2C

>>4
counter-counterexample: propane at −42.09°C

>>5
That... doesn't make sense.  Your "counter-counterexample" fits in with his rule of thumb.  It doesn't validate his claim [does support its possible validity though] or invalidate mine.