1. Thermodynamic Degrees of Freedom for Gases

By the equipartition theorem, internal energy per mole of gas equals c_v T, where T is absolute temperature and the specific heat at constant volume is c_v = (f)(R/2). R = 8.314 J/(K mol) is the universal gas constant, and "f" is the number of thermodynamic (quadratic) degrees of freedom, counting the number of ways in which energy can occur.

Any atom or molecule has three degrees of freedom associated with translational motion (kinetic energy) of the center of mass with respect to the x, y, and z axes. These are the only degrees of freedom for a monoatomic species, such as noble gas atoms.

For a structure consisting of two or more atoms, the whole structure also has rotational kinetic energy, where the whole structure turns about an axis. A linear molecule, where all atoms lie along a single axis, such as any diatomic molecule and some other molecules like carbon dioxide (CO₂), has two rotational degrees of freedom, because it can rotate about either of two axes perpendicular to the molecular axis. A nonlinear molecule, where the atoms do not lie along a single axis, like water (H₂O), has three rotational degrees of freedom, because it can rotate around any of three perpendicular axes. In special cases, such as adsorbed large molecules, the rotational degrees of freedom can be limited to only one.^[1] https://handwiki.org/wiki/index.php?curid=1714013

A structure consisting of two or more atoms also has vibrational energy, where the individual atoms move with respect to one another. A diatomic molecule has one molecular vibration mode: the two atoms oscillate back and forth with the chemical bond between them acting as a spring. A molecule with N atoms has more complicated modes of molecular vibration, with 3N − 5 vibrational modes for a linear molecule and 3N − 6 modes for a nonlinear molecule.^[2] As specific examples, the linear CO₂ molecule has 4 modes of oscillation,^[3] and the nonlinear water molecule has 3 modes of oscillation^[4] Each vibrational mode has two energy terms: the kinetic energy of the moving atoms and the potential energy of the spring-like chemical bond(s). Therefore, the number of vibrational energy terms 2(3N − 5) for a linear molecule and 2(3N − 6) modes for a nonlinear molecule.

Both the rotational and vibrational modes are quantized, requiring a minimum temperature to be activated.^[5] The "rotational temperature" to activate the rotational degrees of freedom is less than 100 K for many gases. For N₂ and O₂, it is less than 3 K.^[6] The "vibrational temperature" necessary for substantial vibration is between 10³ K and 10⁴ K, 3521 K for N₂ and 2156 K for O₂.^[6] Typical atmospheric temperatures are not high enough to activate vibration in N₂ and O₂, which comprise most of the atmosphere. (See the next figure.) However, the much less abundant greenhouse gases keep the troposphere warm by absorbing infrared from the Earth's surface, which excites their vibrational modes.^[7] Much of this energy is reradiated back to the surface in the infrared through the "greenhouse effect."

Because room temperature (≈298 K) is over the typical rotational temperature but lower than the typical vibrational temperature, only the translational and rotational degrees of freedom contribute, in equal amounts, to the heat capacity ratio. This is why γ≈5/3 for monatomic gases and γ≈7/5 for diatomic gases at room temperature.^[6]

Graph of the specific heat of dry air at constant volume, c_v, as a function of temperature numerical values are taken from the table at Air - Specific Heat at Constant Pressure and Varying Temperature.^[8] Those values have units of J/(K kg), so reference lines at plotted (5/2) R_d and (7/2) R_d, where R_d = R/M_d is the gas constant for dry air, R = 8.314 J/(K mol) is the universal gas constant, and M_d = 28.965369 g/mol is the molar mass of dry air.^[9] At T = 140, 160, 200, 220, 320, 340, 360, 380 K, c_v = 718.4, 717.2, 716.3, 716.3, 719.2, 720.6, 722.3, 724.3 J/(K kg). Thus, for 140 K < T < 360 K, c_v differs from (5/2) R_d by less than 1%. https://handwiki.org/wiki/index.php?curid=1503907

Because air is dominated by diatomic gases nitrogen and oxygen, its molar internal energy is close to c_v T = (5/2)RT, determined by the 5 degrees of freedom exhibited by diatomic gases.^[10] See the graph at right. For 140 K < T < 380 K, c_v differs from (5/2) R_d by less than 1%. Only at temperatures well above temperatures in the troposphere and stratosphere do some molecules have enough energy to activate the vibrational modes of N₂ and O₂. The specific heat at constant volume, c_v, increases slowly toward (7/2) R as temperature increases above T = 400 K, where c_v is 1.3% above (5/2) R_d = 717.5 J/(K kg).

Counting the minimum number of co-ordinates to specify a position

One can also count degrees of freedom using the minimum number of coordinates required to specify a position. This is done as follows:

1. For a single particle we need 2 coordinates in a 2-D plane to specify its position and 3 coordinates in 3-D space. Thus its degree of freedom in a 3-D space is 3.
2. For a body consisting of 2 particles (ex. a diatomic molecule) in a 3-D space with constant distance between them (let's say d) we can show (below) its degrees of freedom to be 5.

Let's say one particle in this body has coordinate (x₁, y₁, z₁) and the other has coordinate (x₂, y₂, z₂) with z₂ unknown. Application of the formula for distance between two coordinates

[math]\displaystyle{ d=\sqrt{(x_2-x_1)^2+(y_2-y_1)^2+(z_2-z_1)^2} }[/math]

results in one equation with one unknown, in which we can solve for z₂. One of x₁, x₂, y₁, y₂, z₁, or z₂ can be unknown.

Contrary to the classical equipartition theorem, at room temperature, the vibrational motion of molecules typically makes negligible contributions to the heat capacity. This is because these degrees of freedom are frozen because the spacing between the energy eigenvalues exceeds the energy corresponding to ambient temperatures (k_BT).^[6]

2. Independent Degrees of Freedom

The set of degrees of freedom X₁, ... , X_N of a system is independent if the energy associated with the set can be written in the following form:

[math]\displaystyle{ E = \sum_{i=1}^N E_i(X_i), }[/math]

where E_i is a function of the sole variable X_i.

example: if X₁ and X₂ are two degrees of freedom, and E is the associated energy:

• If [math]\displaystyle{ E = X_1^4 + X_2^4 }[/math], then the two degrees of freedom are independent.
• If [math]\displaystyle{ E = X_1^4 + X_1 X_2 + X_2^4 }[/math], then the two degrees of freedom are not independent. The term involving the product of X₁ and X₂ is a coupling term that describes an interaction between the two degrees of freedom.

For i from 1 to N, the value of the ith degree of freedom X_i is distributed according to the Boltzmann distribution. Its probability density function is the following:

[math]\displaystyle{ p_i(X_i) = \frac{e^{-\frac{E_i}{k_B T}}}{\int dX_i \, e^{-\frac{E_i}{k_B T}}} }[/math],

In this section, and throughout the article the brackets [math]\displaystyle{ \langle \rangle }[/math] denote the mean of the quantity they enclose.

The internal energy of the system is the sum of the average energies associated with each of the degrees of freedom:

[math]\displaystyle{ \langle E \rangle = \sum_{i=1}^N \langle E_i \rangle. }[/math]

3. Quadratic Degrees of Freedom

A degree of freedom X_i is quadratic if the energy terms associated with this degree of freedom can be written as

[math]\displaystyle{ E = \alpha_i\,\,X_i^2 + \beta_i \,\, X_i Y }[/math],

where Y is a linear combination of other quadratic degrees of freedom.

example: if X₁ and X₂ are two degrees of freedom, and E is the associated energy:

• If [math]\displaystyle{ E = X_1^4 + X_1^3 X_2 + X_2^4 }[/math], then the two degrees of freedom are not independent and non-quadratic.
• If [math]\displaystyle{ E = X_1^4 + X_2^4 }[/math], then the two degrees of freedom are independent and non-quadratic.
• If [math]\displaystyle{ E = X_1^2 + X_1 X_2 + 2X_2^2 }[/math], then the two degrees of freedom are not independent but are quadratic.
• If [math]\displaystyle{ E = X_1^2 + 2X_2^2 }[/math], then the two degrees of freedom are independent and quadratic.

For example, in Newtonian mechanics, the dynamics of a system of quadratic degrees of freedom are controlled by a set of homogeneous linear differential equations with constant coefficients.

3.1. Quadratic and Independent Degree of Freedom

X₁, ... , X_N are quadratic and independent degrees of freedom if the energy associated with a microstate of the system they represent can be written as:

[math]\displaystyle{ E = \sum_{i=1}^N \alpha_i X_i^2 }[/math]

3.2. Equipartition Theorem

In the classical limit of statistical mechanics, at thermodynamic equilibrium, the internal energy of a system of N quadratic and independent degrees of freedom is:

[math]\displaystyle{ U = \langle E \rangle = N\,\frac{k_B T}{2} }[/math]

Here, the mean energy associated with a degree of freedom is:

[math]\displaystyle{ \langle E_i \rangle = \int dX_i\,\,\alpha_i X_i^2\,\, p_i(X_i) = \frac{\int dX_i\,\,\alpha_i X_i^2\,\, e^{-\frac{\alpha_i X_i^2}{k_B T}}}{\int dX_i\,\, e^{-\frac{\alpha_i X_i^2}{k_B T}}} }[/math]

[math]\displaystyle{ \langle E_i \rangle = \frac{k_B T}{2}\frac{\int dx\,\,x^2\,\, e^{-\frac{x^2}{2}}}{\int dx\,\, e^{-\frac{x^2}{2}}} = \frac{k_B T}{2} }[/math]

Since the degrees of freedom are independent, the internal energy of the system is equal to the sum of the mean energy associated with each degree of freedom, which demonstrates the result.

4. Generalizations

The description of a system's state as a point in its phase space, although mathematically convenient, is thought to be fundamentally inaccurate. In quantum mechanics, the motion degrees of freedom are superseded with the concept of wave function, and operators which correspond to other degrees of freedom have discrete spectra. For example, intrinsic angular momentum operator (which corresponds to the rotational freedom) for an electron or photon has only two eigenvalues. This discreteness becomes apparent when action has an order of magnitude of the Planck constant, and individual degrees of freedom can be distinguished.

The content is sourced from: https://handwiki.org/wiki/Chemistry:Degrees_of_freedom_(physics_and_chemistry)