Changes of Internal Energy un open system My professor says the internal energy of a system can be calculated as $U=n T c_v$. Now I always thought that we could only calculate a change in internal energy $\Delta U = n c_v \Delta T$. 

Following this idea, he says that a recipient that contains gas and loses a certain number of moles at constant temperautre undergoes a change in internal energy of $\Delta U = T c_v \Delta n$.

I've never seen any of this in any book. I believe he is assuming that the internal energy at 0 Kelvin is zero, which I believe is not true. However, in the case of the recipient losing gas,I wouldn't know how to calculate $\Delta U$.

Any thoughts? thanks!
Suppose you assign an reference state for internal energy such that the internal energy per mole u of the gas is zero at $T=T_r$.  This reference state is going to be held fixed for the material both entering or leaving the open system, as well as the material within the system at any time.  Then, in the initial state of a constant-temperature system, $U_{init}=n_{init}C_v(T-T_r)$ and, in the final state, $U_{final}=n_{final}C_v(T-T_r)$.  So, $$\Delta U=\Delta nC_v(T-T_r)$$Typically, in the overall energy balance on the system, including entering and exiting streams, $T_r$ will cancel out (just as it would for a closed system).  

Please note, however, that if chemical reactions are occurring, the equation for   the internal energy and the specification of the reference state has to be extended to take this into account (using the concept of "internal energy of formation").