- #1
Matthew Marko
- 7
- 0
I am looking over the kinetic theory of gases. It is most commonly described as
U = (3/2)*N*k*T = (3/2)*mass*R*T
for a monatomic gas, assuming the gas is ideal. This is based on the derivation, where ultimately
(3/2)*P*V = N*K = total kinetic energy of particles.
My question, for a real gas, such as following Van der Waal, or even a liquid, is it reasonable to assume:
U = (3/2)*P*V
for the internal energy, regardless of the phase? As far as I can derive, this should be valid, but I welcome other responses. Original references would be much appreciated as well.
U = (3/2)*N*k*T = (3/2)*mass*R*T
for a monatomic gas, assuming the gas is ideal. This is based on the derivation, where ultimately
(3/2)*P*V = N*K = total kinetic energy of particles.
My question, for a real gas, such as following Van der Waal, or even a liquid, is it reasonable to assume:
U = (3/2)*P*V
for the internal energy, regardless of the phase? As far as I can derive, this should be valid, but I welcome other responses. Original references would be much appreciated as well.