Heat capacity and expansion work

Description
this lecture is based on heat capacity. The first law, a process that takes a gas from p1, V1, T to p2, V2, T examined for various paths. And what you'll find is that the maximum work out is obtain for a reversible path. We'll then look at the quantity, internal energy, which we define through the first law, and we think of it as a function of two variables T and V. And whenever we say something like that, we'll be able to write a differential, the partial of u, with respect to T at constant V, dT, plus the partial of u with respect to V at constant T dV. Also about isothermal expansion, the Joule expansion. So, if you have an isothermal process for an ideal gas, the energy doesn't change. q plus w is equal to zero for any isothermal process. And you also see that du then could be written as Cv dT for an ideal gas always. This is not generally true. If you have a real gas and you write du is Cv dT.Prof. Keith A. Nelson and Prof. Moungi Bawendi, 5.60 Thermodynamics & Kinetics, Spring 2008, Massachusetts Institute of Technology: MIT OpenCourseWare), http://ocw.mit.edu (Accessed 2 january 2011). License: Creative Commons BY-NC-SA: http://ocw.mit.edu/terms/#cc