Materials Science and Engineering/Equations

Notation

Conjugate variables
p	Pressure	V	Volume
T	Temperature	S	Entropy
μ	Chemical potential	N	Particle number

Thermodynamic potentials
U	Internal energy	A	Helmholtz free energy
H	Enthalpy	G	Gibbs free energy

Material properties
ρ	Density
CV	Heat capacity (constant volume)
Cp	Heat capacity (constant pressure)
${\beta }_T$	Isothermal compressibility
${\beta }_S$	Adiabatic compressibility
$\alpha$	Coefficient of thermal expansion

Other conventional variables
δw	infinitesimal amount of Mechanical Work
δq	infinitesimal amount of Heat

Constants
kB	Boltzmann constant
R	Ideal gas constant

Equations

Laws of Thermodynamics

First Law of Thermodynamics:

$dU=\delta Q-\delta W$

Second Law of Thermodynamics:

$\int \frac{\delta Q}{T}\ge 0$

Fundamental Equations

The Fundamental Equation:

$dU\le TdS-pdV+\sum _{i=1}^p{\mu }_{i}d{N}_i$

The equation may be seen as a particular case of the chain rule:

$dU={\left(\frac{\partial U}{\partial S}\right)}_{V,\{N_i\}}dS+{\left(\frac{\partial U}{\partial V}\right)}_{S,\{N_i\}}dV+\sum _i{\left(\frac{\partial U}{\partial N_i}\right)}_{S,V,\{N_{j\ne i}\}}d{N}_i$

from which the following identifications can be made:

${\left(\frac{\partial U}{\partial S}\right)}_{V,\{N_i\}}=T$

${\left(\frac{\partial U}{\partial V}\right)}_{S,\{N_i\}}=-p$

${\left(\frac{\partial U}{\partial N_i}\right)}_{S,V,\{N_{j\ne i}\}}={\mu }_i$

These equations are known as "equations of state" with respect to the internal energy.

Thermodynamic Potentials

Thermodynamic Potentials:

Name	Formula	Natural variables
Internal energy	$U$	$S,V,\{N_i\}$
Helmholtz free energy	$A=U-TS$	$T,V,\{N_i\}$
Enthalpy	$H=U+pV$	$S,p,\{N_i\}$
Gibbs free energy	$G=U+pV-TS$	$T,p,\{N_i\}$

For the above four potentials, the fundamental equations are expressed as:

$dU(S,V,N_i)=TdS-pdV+\sum _i{\mu }_{i}d{N}_i$

$dA(T,V,N_i)=-SdT-pdV+\sum _i{\mu }_{i}d{N}_i$

$dH(S,p,N_i)=TdS+Vdp+\sum _i{\mu }_{i}d{N}_i$

$dG(T,p,N_i)=-SdT+Vdp+\sum _i{\mu }_{i}d{N}_i$

Euler Integrals:

Because all of natural variables of the internal energy U are extensive quantities, it follows from Euler's homogeneous function theorem that

$U=TS-pV+\sum _i{\mu }_i{N}_i$

Substituting into the expressions for the other main potentials we have the following expressions for the thermodynamic potentials:

$A=-pV+\sum _i{\mu }_i{N}_i$

$H=TS+\sum _i{\mu }_i{N}_i$

$G=\sum _i{\mu }_i{N}_i$

Note that the Euler integrals are sometimes also referred to as fundamental equations.

Gibbs Duhem Relationship:

Differentiating the Euler equation for the internal energy and combining with the fundamental equation for internal energy, it follows that:

$0=SdT-Vdp+\sum _i{N}_{i}d{\mu }_i$

which is known as the Gibbs-Duhem relationship. The Gibbs-Duhem is a relationship among the intensive parameters of the system. It follows that for a simple system with r components, there will be r+1 independent parameters, or degrees of freedom. For example, a simple system with a single component will have two degrees of freedom, and may be specified by only two parameters, such as pressure and volume for example. The law is named after Josiah Gibbs and Pierre Duhem.

Materials Properties

Compressibility: At constant temperature or constant entropy

${\beta }_{T\text{ or }S}=-\frac{1}{V}{\left(\frac{\partial V}{\partial p}\right)}_{T,N\text{ or }S,N}$

Heat Capacity at Constant Pressure:

$C_p={\left(\frac{\partial U}{\partial T}\right)}_p+p{\left(\frac{\partial V}{\partial T}\right)}_p={\left(\frac{\partial H}{\partial T}\right)}_p=T{\left(\frac{\partial S}{\partial T}\right)}_p$

Heat Capacity at Constant Volume:

$C_V={\left(\frac{\partial U}{\partial T}\right)}_V=T{\left(\frac{\partial S}{\partial T}\right)}_V$

Coefficient of Thermal Expansion:

${\alpha }_p=\frac{1}{V}{\left(\frac{\partial V}{\partial T}\right)}_p$

Maxwell Relations:

Maxwell relations are equalities involving the second derivatives of thermodynamic potentials with respect to their natural variables. They follow directly from the fact that the order of differentiation does not matter when taking the second derivative. The four most common Maxwell relations are:

${\left(\frac{\partial T}{\partial V}\right)}_{S,N}=-{\left(\frac{\partial p}{\partial S}\right)}_{V,N}$		${\left(\frac{\partial T}{\partial p}\right)}_{S,n}={\left(\frac{\partial V}{\partial S}\right)}_{p,N}$
${\left(\frac{\partial T}{\partial V}\right)}_{p,N}=-{\left(\frac{\partial p}{\partial S}\right)}_{T,N}$		${\left(\frac{\partial T}{\partial p}\right)}_{V,N}={\left(\frac{\partial V}{\partial S}\right)}_{T,N}$

Processes

Incremental Processes:

$dU=TdS-pdV+\mu dN$

$dA=-SdT-pdV+\mu dN$

$dG=-SdT+Vdp+\mu dN=\mu dN+Nd\mu$

$dH=TdS+Vdp+\mu dN$

Equation Table for an Ideal Gas ($P{V}^m=constant$):

	Constant Pressure	Constant Volume	Isothermal	Adiabatic
Variable	$\mathrm{\Delta }p=0$	$\mathrm{\Delta }V=0$	$\mathrm{\Delta }T=0$	$q=0$
$m$	$0$	$\mathrm{\infty }$	$1$	$\gamma =\frac{C_p}{C_V}$
Work $\begin{array}{c}w=-\underset{V_1}{\overset{V_2}{\int }}pdV\end{array}$	$-p(V_2-V_1)$	$0$	$-nRT\ln \frac{V_2}{V_1}$	$C_V(T_2-T_1)$
Heat Capacity, $C$	$C_p=(5/2)nR$	$C_V=(3/2)nR$	$C_p$ or $C_V$	$C_p$ or $C_V$
Internal Energy, $\mathrm{\Delta }U=3/2*nR\mathrm{\Delta }T$	$q+w$ $q_p+p\mathrm{\Delta }V$	$q$ $C_V(T_2-T_1)$	$0$ $q=-w$	$w$ $C_V(T_2-T_1)$
Enthalpy, $\mathrm{\Delta }H$ $H=U+pV$	$C_p(T_2-T_1)$	$q_V+V\mathrm{\Delta }P$	$0$	$C_p(T_2-T_1)$
Entropy $\begin{array}{c}\mathrm{\Delta }S=-\underset{T_1}{\overset{T_2}{\int }}\frac{C}{T}dT\end{array}$	$C_p\ln \frac{T_2}{T_1}$	$C_V\ln \frac{T_2}{T_1}$	$nR\ln \frac{V_2}{V_1}$ $\frac{q}{T}$	$0$