Derivation of polytropic process equation I know that a polytropic process equation is often the result of an empirical fit of a P-V curve that allows one to derive some nice analytical equations for the process.  Is there actually a derivation for the polytropic process equation?
 A: Indeed, the general polytropic equation $pV^n=C$ is meant as a fit to describe a wide variety of situations - but the general situations don't have to exactly obey any polytropic equation with any $n$, anyway (because the right $n$ depends on $p$ and/or $V$), so there is nothing to derive.
A major, general enough exception is the adiabatic equation $pV^\gamma = C$. It only differs by using the name $\gamma$ for $n$ where $\gamma = C_P/C_V$, the ratio of heat capacities at constant pressure and volume, respectively. The adiabatic process is one in which no heat is transferred between the gas and the environment, so all the work being used or consumed is used to change the internal thermal energy of the gas. Nevertheless, $\gamma$ can have many different values such as $5/3$ etc. Microscopically, the value is linked to a function of the degrees of freedom of a single (average) molecule.
In that case, the derivation of the adiabatic equation - based on $\alpha p \,dV = dU $ - is here:

http://en.wikipedia.org/wiki/Adiabatic_process#Derivation_of_continuous_formula

A: From the first law of thermodynamics;
$$dU+dW=dQ$$
As;
$$C_V = \frac {dU}{dT},$$
$$C=\frac {dQ}{dT},$$
$$dW=PdV,$$
We have;
$$C_VdT + PdV = CdT$$
Multiplying throughout by $R$ ;
$$C_V.RdT + R.PdV = R.CdT$$
By the ideal gas law;
$$PV=RT$$
$$→PdV+VdP=RdT$$
Hence;
$$C_V(PdV+VdP) + R.PdV=R.CdT$$
$$→PdV(C_V+R) + C_V.VdP = R.CdT$$
But $C_P - C_V = R$. Hence;
$$C_P.PdV + C_V.VdP = R.CdT$$
$$→C_V.VdP = R.CdT - C_P.PdV$$
$$=(C_P-C_V).CdT - C_P.PdV$$
Dividing throughout by $C_V$ , noting that $\frac {C_P}{C_V} = \gamma$ and rearranging;
$$VdP = -[(1-\gamma)CdT + \gamma .PdV]$$
$$=-[(1-\gamma)dQ + \gamma .dW]$$
$$=-\left[(1-\gamma)\frac {dQ}{dW} + \gamma \right].dW$$
$$-\left[(1-\gamma)\frac {dQ}{dW} + \gamma \right].PdV$$
Noting that for a polytropic process $\frac {dQ}{dW} = \text {constant} = K$ and rearranging;
$$\frac {dP}{P} + [(1-\gamma)K + \gamma ].\frac {dV}{V} = 0$$
Integrating both sides , we have;
$$\ln P + [(1-\gamma)K + \gamma ].\ln V = C' = \ln C$$
$$~PV^{(1-\gamma)K + \gamma } = C$$
In a simplified way , we can write;
$$PV^n = \text {constant}$$
A: In addition to Lubos’ answer, it can be said that the polytropic exponent n is a representation of our ignorance in the actual transformation undergone by a gas.
There are basically two limiting cases : adiabatic and isothermal.
The later is characterized by $PV=Cst$ , ie $n=1$, while the former has $n= \gamma$.
A real process is never perfectly isothermal or adiabatic, and this results in a wide range of values possible for $n$.
A: Yes, there is an explicit mathematical derivation.  The basis of this derivation is that the ratio of heat transfer to work (dq/dw -- the "energy transfer ratio") in a polytropic process is constant.  Do a Google search on "polytropic energy transfer ratio" and you'll find a link to a useful article in the International Journal of Mechanical Engineering Education.
