Table of thermodynamic equations

For list of mathematical notation used in these equations, see mathematical notation.

Branches

Equilibrium / Non-equilibrium

State
Equation of state Ideal gas Real gas State of matter Equilibrium Control volume Instruments
Processes
Isobaric Isochoric Isothermal Adiabatic Isentropic Isenthalpic Quasistatic Polytropic Free expansion Reversibility Irreversibility Endoreversibility
Cycles
Heat engines Heat pumps Thermal efficiency

System properties

Note: Conjugate variables in italics

Functions of state
Property diagrams Intensive and extensive properties
Temperature / Entropy (introduction) Pressure / Volume Chemical potential / Particle number Vapor quality Reduced properties
Process functions
Work Heat

Material properties

Property databases

Specific heat capacity

c=

$T$	$\partial S$
$N$	$\partial T$

Compressibility

\beta =-

$1$	$\partial V$
$V$	$\partial p$

Thermal expansion

\alpha =

$1$	$\partial V$
$V$	$\partial T$

Equations

Potentials

Internal energy
$U(S,V)$
Enthalpy
$H(S,p)=U+pV$
Helmholtz free energy
$A(T,V)=U-TS$
Gibbs free energy
$G(T,p)=H-TS$

History
Culture

History
General Heat Entropy Gas laws "Perpetual motion" machines
Philosophy
Entropy and time Entropy and life Brownian ratchet Maxwell's demon Heat death paradox Loschmidt's paradox Synergetics
Theories
Caloric theory Theory of heat Vis viva ("living force") Mechanical equivalent of heat Motive power
Key publications
"An Experimental Enquiry Concerning ... Heat" "On the Equilibrium of Heterogeneous Substances" "Reflections on the Motive Power of Fire"
Timelines
Thermodynamics Heat engines
Art Education
Maxwell's thermodynamic surface Entropy as energy dispersal

Scientists

Book:Thermodynamics

Main article: List of thermodynamic properties

This article is a summary of common equations and quantities in thermodynamics (see thermodynamic equations for more elaboration). SI units are used for absolute temperature, not Celsius or Fahrenheit.

Definitions

Main articles: List of thermodynamic properties, Thermodynamic potential, Free entropy, Defining equation (physical chemistry)

Many of the definitions below are also used in the thermodynamics of chemical reactions.

General basic quantities

Quantity (Common Name/s)	(Common) Symbol/s	SI Units	Dimension
Number of molecules	N	dimensionless	dimensionless
Number of moles	n	mol	[N]
Temperature	T	K	[Θ]
Heat Energy	Q, q	J	[M][L]²[T]⁻²
Latent Heat	Q_L	J	[M][L]²[T]⁻²

General derived quantities

Quantity (Common Name/s)	(Common) Symbol/s	Defining Equation	SI Units	Dimension
Thermodynamic beta, Inverse temperature	β	$\beta = 1/k_B T \,\!$	J⁻¹	[T]²[M]⁻¹[L]⁻²
Thermodynamic Temperature	τ	$\tau =k_{B}T\,\!$ $\tau =k_{B}\left(\partial U/\partial S\right)_{{N}}\,\!$ $1/\tau =1/k_{B}\left(\partial S/\partial U\right)_{{N}}\,\!$	J	[M] [L]² [T]⁻²
Entropy	S	$S = -k_B\sum_i p_i\ln p_i$ $S=\left(\partial F/\partial T\right)_{{V}}\,\!$ , $S=\left(\partial G/\partial T\right)_{{N,P}}\,\!$	J K⁻¹	[M][L]²[T]⁻² [Θ]⁻¹
Pressure	P	$P=-\left(\partial F/\partial V\right)_{{T,N}}\,\!$ $P=-\left(\partial U/\partial V\right)_{{S,N}}\,\!$	Pa	M L⁻¹T⁻²
Internal Energy	U	$U = \sum_i E_i \!$	J	[M][L]²[T]⁻²
Enthalpy	H	$H = U+pV\,\!$	J	[M][L]²[T]⁻²
Partition Function	Z		dimensionless	dimensionless
Gibbs free energy	G	$G = H - TS \,\!$	J	[M][L]²[T]⁻²
Chemical potential (of component i in a mixture)	μ_i	$\mu _{i}=\left(\partial U/\partial N_{i}\right)_{{N_{{j\neq i}},S,V}}\,\!$ $\mu _{i}=\left(\partial F/\partial N_{i}\right)_{{T,V}}\,\!$ , where F is not proportional to N because μ_i depends on pressure. $\mu _{i}=\left(\partial G/\partial N_{i}\right)_{{T,P}}\,\!$ , where G is proportional to N (as long as the molar ratio composition of the system remains the same) because μ_i depends only on temperature and pressure and composition. $\mu _{i}/\tau =-1/k_{B}\left(\partial S/\partial N_{i}\right)_{{U,V}}\,\!$	J	[M][L]²[T]⁻²
Helmholtz free energy	A, F	$F = U - TS \,\!$	J	[M][L]²[T]⁻²
Landau potential, Landau Free Energy, Grand potential	Ω, Φ_G	$\Omega = U - TS - \mu N\,\!$	J	[M][L]²[T]⁻²
Massieu Potential, Helmholtz free entropy	Φ	$\Phi = S - U/T \,\!$	J K⁻¹	[M][L]²[T]⁻² [Θ]⁻¹
Planck potential, Gibbs free entropy	Ξ	$\Xi = \Phi - pV/T \,\!$	J K⁻¹	[M][L]²[T]⁻² [Θ]⁻¹

Thermal properties of matter

Main Articles: Heat capacity, Thermal expansion

Quantity (common name/s)	(Common) symbol/s	Defining equation	SI units	Dimension
General heat/thermal capacity	C	$C = \partial Q/\partial T\,\!$	J K ⁻¹	[M][L]²[T]⁻² [Θ]⁻¹
Heat capacity (isobaric)	C_p	$C_{p} = \partial H/\partial T\,\!$	J K ⁻¹	[M][L]²[T]⁻² [Θ]⁻¹
Specific heat capacity (isobaric)	C_mp	$C_{mp} = \partial^2 Q/\partial m \partial T \,\!$	J kg⁻¹ K⁻¹	[L]²[T]⁻² [Θ]⁻¹
Molar specific heat capacity (isobaric)	C_np	$C_{np} = \partial^2 Q/\partial n \partial T \,\!$	J K ⁻¹ mol⁻¹	[M][L]²[T]⁻² [Θ]⁻¹ [N]⁻¹
Heat capacity (isochoric/volumetric)	C_V	$C_{V} = \partial Q/\partial T \,\!$	J K ⁻¹	[M][L]²[T]⁻² [Θ]⁻¹
Specific heat capacity (isochoric)	C_mV	$C_{mV} = \partial^2 Q/\partial m \partial T \,\!$	J kg⁻¹ K⁻¹	[L]²[T]⁻² [Θ]⁻¹
Molar specific heat capacity (isochoric)	C_nV	$C_{nV} = \partial^2 Q/\partial n \partial T \,\!$	J K ⁻¹ mol⁻¹	[M][L]²[T]⁻² [Θ]⁻¹ [N]⁻¹
Specific latent heat	L	$L = \partial Q/ \partial m \,\!$	J kg⁻¹	[L]²[T]⁻²
Ratio of isobaric to isochoric heat capacity, heat capacity ratio, adiabatic index	γ	$\gamma = C_p/C_V = c_p/c_V = C_{mp}/C_{mV} \,\!$	dimensionless	dimensionless

Thermal transfer

Main article: Thermal conductivity

Quantity (common name/s)	(Common) symbol/s	Defining equation	SI units	Dimension
Temperature gradient	No standard symbol	$\nabla T \,\!$	K m⁻¹	[Θ][L]⁻¹
Thermal conduction rate, thermal current, thermal/heat flux, thermal power transfer	P	$P = \mathrm{d} Q/\mathrm{d} t \,\!$	W = J s⁻¹	[M] [L]² [T]⁻³
Thermal intensity	I	$I = \mathrm{d} P/\mathrm{d} A$	W m⁻²	[M] [T]⁻³
Thermal/heat flux density (vector analogue of thermal intensity above)	q	$Q = \iint \mathbf{q} \cdot \mathrm{d}\mathbf{S}\mathrm{d} t \,\!$	W m⁻²	[M] [T]⁻³

Equations

The equations in this article are classified by subject.By Danish

Phase transitions

Physical situation	Equations
Adiabatic transition	$\Delta Q=0,\quad \Delta U=-\Delta W\,\!$
Isothermal transition	$\Delta U=0,\quad \Delta W=\Delta Q\,\!$ For an ideal gas $W=kTN \ln(V_2/V_1)\,\!$
Isobaric transition	p₁ = p₂, p = constant $\Delta W = p \Delta V, \quad \Delta Q = \Delta U + p \delta V\,\!$
Isochoric transition	V₁ = V₂, V = constant $\Delta W = 0, \quad \Delta Q = \Delta U\,\!$
Adiabatic expansion	$p_1 V_1^{\gamma} = p_2 V_2^{\gamma}\,\!$ $T_1 V_1^{\gamma - 1} = T_2 V_2^{\gamma - 1} \,\!$
Free expansion	$\Delta U = 0\,\!$
Work done by an expanding gas	Process $\Delta W = \int_{V_1}^{V_2} p \mathrm{d}V \,\!$ Net Work Done in Cyclic Processes $\Delta W = \oint_\mathrm{cycle} p \mathrm{d}V \,\!$

Kinetic theory

Ideal gas equations
Physical situation	Nomenclature	Equations
Ideal gas law	p = pressure V = volume of container T = temperature n = number of moles R = Gas constant N = number of molecules k = Boltzmann's constant	$pV = nRT = kTN\,\!$ $\frac{p_1 V_1}{p_2 V_2} = \frac{n_1 T_1}{n_2 T_2} = \frac{N_1 T_1}{N_2 T_2} \,\!$
Pressure of an ideal gas	m = mass of one molecule M_m = molar mass	$p = \frac{Nm \langle v^2 \rangle}{3V} = \frac{nM_m \langle v^2 \rangle}{3V} = \frac{1}{3}\rho \langle v^2 \rangle \,\!$

Ideal gas


Quantity	General Equation	Isobaric Δp = 0	Isochoric ΔV = 0	Isothermal ΔT = 0	Adiabatic $Q=0$
Work W	$\delta W=-pdV\;$	$-p\Delta V\;$	$0\;$	$-nRT\ln {\frac {V_{2}}{V_{1}}}\;$ $nRT\ln {\frac {P_{1}}{P_{2}}}\;$	${\frac {PV^{\gamma }(V_{f}^{{1-\gamma }}-V_{i}^{{1-\gamma }})}{1-\gamma }}=C_{V}\left(T_{2}-T_{1}\right)$
Heat Capacity C	(as for real gas)	$C_p = \frac{5}{2}nR\;$ (for monatomic ideal gas) $C_p = \frac{7}{2}nR \;$ (for diatomic ideal gas)	$C_V = \frac{3}{2}nR \;$ (for monatomic ideal gas) $C_{V}={\frac {5}{2}}nR\;$ (for diatomic ideal gas)
Internal Energy ΔU	$\Delta U = C_v \Delta T\;$	$Q + W\;$ $Q_p - p\Delta V\;$	$Q\;$ $C_V\left ( T_2-T_1 \right )\;$	$0\;$ $Q=-W\;$	$W\;$ $C_V\left ( T_2-T_1 \right )\;$
Enthalpy ΔH	$H=U+pV\;$	$C_p\left ( T_2-T_1 \right )\;$	$Q_V+V\Delta p\;$	$0\;$	$C_p\left ( T_2-T_1 \right )\;$
Entropy Δs	$\Delta S = C_v \ln{T_2 \over T_1} + nR \ln{V_2 \over V_1}$ $\Delta S = C_p \ln{T_2 \over T_1} - nR \ln{p_2 \over p_1}$ ^[1]	$C_p\ln\frac{T_2}{T_1}\;$	$C_{V}\ln {\frac {T_{2}}{T_{1}}}\;$	$nR\ln\frac{V_2}{V_1}\;$ $\frac{Q}{T}\;$	$C_{p}\ln {\frac {V_{2}}{V_{1}}}+C_{V}\ln {\frac {p_{2}}{p_{1}}}=0\;$
Constant	$\;$	$\frac{V}{T}\;$	$\frac{p}{T}\;$	$p V\;$	$p V^\gamma\;$

Entropy

$S = k_B (\ln \Omega)$ , where k_B is the Boltzmann constant, and Ω denotes the volume of macrostate in the phase space or otherwise called thermodynamic probability.
$dS = \frac{\delta Q}{T}$ , for reversible processes only

Statistical physics

Below are useful results from the Maxwell–Boltzmann distribution for an ideal gas, and the implications of the Entropy quantity. The distribution is valid for atoms or molecules constituting ideal gases.

Physical situation	Nomenclature	Equations
Maxwell–Boltzmann distribution	v = velocity of atom/molecule, m = mass of each molecule (all molecules are identical in kinetic theory), γ(p) = Lorentz factor as function of momentum (see below) Ratio of thermal to rest mass-energy of each molecule: $\theta = k_B T/mc^2 \,\!$ K₂ is the Modified Bessel function of the second kind.	Non-relativistic speeds $P\left ( v \right )=4\pi\left ( \frac{m}{2\pi k_B T} \right )^{3/2} v^2 e^{-mv^2/2 k_B T} \,\!$ Relativistic speeds (Maxwell-Jüttner distribution) $f(p) = \frac{1}{4 \pi m^3 c^3 \theta K_2(1/\theta)} e^{-\gamma(p)/\theta}$
Entropy Logarithm of the density of states	P_i = probability of system in microstate i Ω = total number of microstates	$S = - k_B\sum_i P_i \ln P_i = k_\mathrm{B}\ln \Omega\,\!$ where: $P_i = 1/\Omega\,\!$
Entropy change		$\Delta S = \int_{Q_1}^{Q_2} \frac{\mathrm{d}Q}{T} \,\!$ $\Delta S = k_B N \ln\frac{V_2}{V_1} + N C_V \ln\frac{T_2}{T_1} \,\!$
Entropic force		$\mathbf{F}_\mathrm{S} = -T \nabla S \,\!$
Equipartition theorem	d_f = degree of freedom	Average kinetic energy per degree of freedom $\langle E_\mathrm{k} \rangle = \frac{1}{2}kT\,\!$ Internal energy $U = d_f \langle E_\mathrm{k} \rangle = \frac{d_f}{2}kT\,\!$

Corollaries of the non-relativistic Maxwell–Boltzmann distribution are below.

Physical situation	Nomenclature	Equations
Mean speed		$\langle v \rangle = \sqrt{\frac{8 k_B T}{\pi m}}\,\!$
Root mean square speed		$v_\mathrm{rms} = \sqrt{\langle v^2 \rangle} = \sqrt{\frac{3k_B T}{m}} \,\!$
Modal speed		$v_\mathrm{mode} = \sqrt{\frac{2k_B T}{m}}\,\!$
Mean free path	σ = Effective cross-section n = Volume density of number of target particles ℓ = Mean free path	$\ell = 1/\sqrt{2} n \sigma \,\!$

Quasi-static and reversible processes

For quasi-static and reversible processes, the first law of thermodynamics is:

dU=\delta Q - \delta W

where δQ is the heat supplied to the system and δW is the work done by the system.

Thermodynamic potentials

Main article: Thermodynamic potentials

Name	Symbol	Formula	Natural variables
Internal energy	$U$	$\int ( T \text{d}S - p \text{d}V + \sum_i \mu_i \text{d}N_i )$	$S, V, \{N_i\}$
Helmholtz free energy	$F$	$U-TS$	$T, V, \{N_i\}$
Enthalpy	$H$	$U+pV$	$S, p, \{N_i\}$
Gibbs free energy	$G$	$U+pV-TS$	$T, p, \{N_i\}$
Landau Potential (Grand potential)	$\Omega$ , $\Phi_\text{G}$	$U - T S -$ $\sum_i\,$ $\mu_i N_i$	$T, V, \{\mu_i\}$

Potential	Differential
Internal energy	$dU\left(S,V,{N_{i}}\right) = TdS - pdV + \sum_{i} \mu_{i} dN_i$
Enthalpy	$dH\left(S,p,{N_{i}}\right) = TdS + Vdp + \sum_{i} \mu_{i} dN_{i}$
Helmholtz free energy	$dF\left(T,V,{N_{i}}\right) = -SdT - pdV + \sum_{i} \mu_{i} dN_{i}$
Gibbs free energy	$dG\left(T,p,{N_{i}}\right) = -SdT + Vdp + \sum_{i} \mu_{i} dN_{i}$

Maxwell's relations

The four most common Maxwell's relations are:

Physical situation	Nomenclature	Equations
Thermodynamic potentials as functions of their natural variables	$U(S,V)\,$ = Internal energy $H(S,P)\,$ = Enthalpy $F(T,V)\,$ = Helmholtz free energy $G(T,P)\,$ = Gibbs free energy	$\left(\frac{\partial T}{\partial V}\right)_S = -\left(\frac{\partial P}{\partial S}\right)_V = \frac{\partial^2 U }{\partial S \partial V}$ $\left(\frac{\partial T}{\partial P}\right)_S = +\left(\frac{\partial V}{\partial S}\right)_P = \frac{\partial^2 H }{\partial S \partial P}$ $+\left(\frac{\partial S}{\partial V}\right)_T = \left(\frac{\partial P}{\partial T}\right)_V = - \frac{\partial^2 F }{\partial T \partial V}$ $-\left(\frac{\partial S}{\partial P}\right)_T = \left(\frac{\partial V}{\partial T}\right)_P = \frac{\partial^2 G }{\partial T \partial P}$

More relations include the following.

$\left ( {\partial S\over \partial U} \right )_{V,N} = { 1\over T }$	$\left ( {\partial S\over \partial V} \right )_{N,U} = { p\over T }$	$\left ( {\partial S\over \partial N} \right )_{V,U} = - { \mu \over T }$
$\left ( {\partial T\over \partial S} \right )_V = { T \over C_V }$	$\left ( {\partial T\over \partial S} \right )_P = { T \over C_P }$
$-\left ( {\partial p\over \partial V} \right )_T = { 1 \over {VK_T} }$

Other differential equations are:

Name	H	U	G
Gibbs–Helmholtz equation	$H = -T^2\left(\frac{\partial \left(G/T\right)}{\partial T}\right)_p$	$U = -T^2\left(\frac{\partial \left(F/T\right)}{\partial T}\right)_V$	$G = -V^2\left(\frac{\partial \left(F/V\right)}{\partial V}\right)_T$
	$\left(\frac{\partial H}{\partial p}\right)_T = V - T\left(\frac{\partial V}{\partial T}\right)_P$	$\left(\frac{\partial U}{\partial V}\right)_T = T\left(\frac{\partial P}{\partial T}\right)_V - P$

Quantum properties

$U = N k_B T^2 \left(\frac{\partial \ln Z}{\partial T}\right)_V ~$
$S = \frac{U}{T} + N * ~ S = \frac{U}{T} + N k_B \ln Z - N k \ln N + Nk ~$ Indistinguishable Particles

where N is number of particles, h is Planck's constant, I is moment of inertia, and Z is the partition function, in various forms:

Degree of freedom	Partition function
Translation	$Z_t = \frac{(2 \pi m k_B T)^\frac{3}{2} V}{h^3}$
Vibration	$Z_v = \frac{1}{1 - e^\frac{-h \omega}{2 \pi k_B T}}$
Rotation	$Z_r = \frac{2 I k_B T}{\sigma (\frac{h}{2 \pi})^2}$ where: σ = 1 (heteronuclear molecules) σ = 2 (homonuclear)

Thermal properties of matter

Coefficients	Equation
Joule-Thomson coefficient	$\mu_{JT} = \left(\frac{\partial T}{\partial p}\right)_H$
Compressibility (constant temperature)	$K_T = -{ 1\over V } \left ( {\partial V\over \partial p} \right )_{T,N}$
Coefficient of thermal expansion (constant pressure)	$\alpha_{p} = \frac{1}{V}\left(\frac{\partial V}{\partial T}\right)_p$
Heat capacity (constant pressure)	$C_p = \left ( {\partial Q_{rev} \over \partial T} \right )_p = \left ( {\partial U \over \partial T} \right )_p + p \left ( {\partial V \over \partial T} \right )_p = \left ( {\partial H \over \partial T} \right )_p = T \left ( {\partial S \over \partial T} \right )_p$
Heat capacity (constant volume)	$C_V = \left ( {\partial Q_{rev} \over \partial T} \right )_V = \left ( {\partial U \over \partial T} \right )_V = T \left ( {\partial S \over \partial T} \right )_V$

Derivation of heat capacity (constant pressure)

Since

\left(\frac{\partial T}{\partial p}\right)_H \left(\frac{\partial p}{\partial H}\right)_T \left(\frac{\partial H}{\partial T}\right)_p = -1

\begin{align} \left(\frac{\partial T}{\partial p}\right)_H & = -\left(\frac{\partial H}{\partial p}\right)_T \left(\frac{\partial T}{\partial H}\right)_p \\ & = \frac{-1}{\left(\frac{\partial H}{\partial T}\right)_p} \left(\frac{\partial H}{\partial p}\right)_T \end{align}

C_p = \left(\frac{\partial H}{\partial T}\right)_p

\Rightarrow \left(\frac{\partial T}{\partial p}\right)_H = -\frac{1}{C_p} \left(\frac{\partial H}{\partial p}\right)_T

Derivation of heat capacity (constant volume)

Since

dU = \delta Q_{rev} - \delta W_{rev} ,

(where δW_rev is the work done by the system),

\delta S = \frac{\delta Q_{rev}}{T}, \delta W_{rev}= p \delta V

d U = T \delta S- p\delta V

\left(\frac{\partial U}{\partial T}\right)_V = T\left(\frac{\partial S}{\partial T}\right)_V - p\left(\frac{\partial V}{\partial T}\right)_V ; C_V = \left(\frac{\partial U}{\partial T}\right)_V

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

Thermal transfer

Physical situation	Nomenclature	Equations
Net intensity emission/absorption	T_external = external temperature (outside of system) T_system = internal temperature (inside system) ε = emmisivity	$I = \sigma \epsilon \left ( T_\mathrm{external}^4 - T_\mathrm{system}^4 \right ) \,\!$
Internal energy of a substance	C_V = isovolumetric heat capacity of substance ΔT = temperature change of substance	$\Delta U = N C_V \Delta T\,\!$
Meyer's equation	C_p = isobaric heat capacity C_V = isovolumetric heat capacity n = number of moles	$C_p - C_V = nR \,\!$
Effective thermal conductivities	λ_i = thermal conductivity of substance i λ_net = equivalent thermal conductivity	Series $\lambda_\mathrm{net} = \sum_j \lambda_j \,\!$ Parallel $\frac{1}{\lambda}_\mathrm{net} = \sum_j \left ( \frac{1}{\lambda}_j \right ) \,\!$

Thermal efficiencies

Physical situation	Nomenclature	Equations
Thermodynamic engines	η = efficiency W = work done by engine Q_H = heat energy in higher temperature reservoir Q_L = heat energy in lower temperature reservoir T_H = temperature of higher temp. reservoir T_L = temperature of lower temp. reservoir	Thermodynamic engine: $\eta = \left \|\frac{W}{Q_H} \right\|\,\!$ Carnot engine efficiency: $\eta_c = 1 - \left \| \frac{Q_L}{Q_H} \right \| = 1-\frac{T_L}{T_H}\,\!$
Refrigeration	K = coefficient of refrigeration performance	Refrigeration performance $K = \left \| \frac{Q_L}{W} \right \| \,\!$ Carnot refrigeration performance $K_C = \frac{\|Q_L\|}{\|Q_H\|-\|Q_L\|} = \frac{T_L}{T_H-T_L}\,\!$

References

↑ Keenan, Thermodynamics, Wiley, New York, 1947
↑ Physical chemistry, P.W. Atkins, Oxford University Press, 1978, ISBN 0 19 855148 7

Atkins, Peter and de Paula, Julio Physical Chemistry, 7th edition, W.H. Freeman and Company, 2002 [ISBN 0-7167-3539-3].
- Chapters 1 - 10, Part 1: Equilibrium.
Bridgman, P.W., Phys. Rev., 3, 273 (1914).
Landsberg, Peter T. Thermodynamics and Statistical Mechanics. New York: Dover Publications, Inc., 1990. (reprinted from Oxford University Press, 1978).
Lewis, G.N., and Randall, M., "Thermodynamics", 2nd Edition, McGraw-Hill Book Company, New York, 1961.
Reichl, L.E., "A Modern Course in Statistical Physics", 2nd edition, New York: John Wiley & Sons, 1998.
Schroeder, Daniel V. Thermal Physics. San Francisco: Addison Wesley Longman, 2000 [ISBN 0-201-38027-7].
Silbey, Robert J., et al. Physical Chemistry. 4th ed. New Jersey: Wiley, 2004.
Callen, Herbert B. (1985). "Thermodynamics and an Introduction to Themostatistics", 2nd Ed., New York: John Wiley & Sons.

External links

Thermodynamic equation calculator

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Table of thermodynamic equations

Definitions

General basic quantities

General derived quantities

Thermal properties of matter

Thermal transfer

Equations

Phase transitions

Kinetic theory

Ideal gas

Entropy

Statistical physics

Quasi-static and reversible processes

Thermodynamic potentials

Maxwell's relations

Quantum properties

Thermal properties of matter

Thermal transfer

Thermal efficiencies

See also

References

External links