Английская Википедия:Heat capacity ratio

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Heat capacity ratio for various gases

Gas	Temp. [°C]	Шаблон:Math
H2	−181	1.597
	−76	1.453
	20	1.410
	100	1.404
	400	1.387
	1000	1.358
	2000	1.318
He	20	1.66
Ar	−180	1.760
	20	1.670
O2	−181	1.450
	−76	1.415
	20	1.400
	100	1.399
	200	1.397
	400	1.394
N2	−181	1.470
Cl2	20	1.340
Ne	19	1.640
Xe	19	1.660
Kr	19	1.680
Hg	360	1.670
H2O	20	1.330
	100	1.324
	200	1.310
CO2	0	1.310
	20	1.300
	100	1.281
	400	1.235
	1000	1.195
CO	20	1.400
NO	20	1.400
N2O	20	1.310
CH4	−115	1.410
	−74	1.350
	20	1.320
NH3	15	1.310
SO2	15	1.290
C2H6	15	1.220
C3H8	16	1.130
Dry air	-15	1.404
	0	1.403
	20	1.400
	200	1.398
	400	1.393
	1000	1.365

In thermal physics and thermodynamics, the heat capacity ratio, also known as the adiabatic index, the ratio of specific heats, or Laplace's coefficient, is the ratio of the heat capacity at constant pressure (Шаблон:Mvar) to heat capacity at constant volume (Шаблон:Mvar). It is sometimes also known as the isentropic expansion factor and is denoted by Шаблон:Math (gamma) for an ideal gas or Шаблон:Mvar (kappa), the isentropic exponent for a real gas. The symbol Шаблон:Math is used by aerospace and chemical engineers.

<math> \gamma = \frac{C_P}{C_V} = \frac{\bar{C}_P}{\bar{C}_V} = \frac{c_P}{c_V}, </math>

where Шаблон:Mvar is the heat capacity, <math>{\bar{C}}</math> the molar heat capacity (heat capacity per mole), and Шаблон:Mvar the specific heat capacity (heat capacity per unit mass) of a gas. The suffixes Шаблон:Mvar and Шаблон:Mvar refer to constant-pressure and constant-volume conditions respectively.

The heat capacity ratio is important for its applications in thermodynamical reversible processes, especially involving ideal gases; the speed of sound depends on this factor.

Thought experiment

To understand this relation, consider the following thought experiment. A closed pneumatic cylinder contains air. The piston is locked. The pressure inside is equal to atmospheric pressure. This cylinder is heated to a certain target temperature. Since the piston cannot move, the volume is constant. The temperature and pressure will rise. When the target temperature is reached, the heating is stopped. The amount of energy added equals Шаблон:Math, with Шаблон:Math representing the change in temperature.

The piston is now freed and moves outwards, stopping as the pressure inside the chamber reaches atmospheric pressure. We assume the expansion occurs without exchange of heat (adiabatic expansion). Doing this work, air inside the cylinder will cool to below the target temperature.

To return to the target temperature (still with a free piston), the air must be heated, but is no longer under constant volume, since the piston is free to move as the gas is reheated. This extra heat amounts to about 40% more than the previous amount added. In this example, the amount of heat added with a locked piston is proportional to Шаблон:Mvar, whereas the total amount of heat added is proportional to Шаблон:Mvar. Therefore, the heat capacity ratio in this example is 1.4.

Another way of understanding the difference between Шаблон:Mvar and Шаблон:Mvar is that Шаблон:Mvar applies if work is done to the system, which causes a change in volume (such as by moving a piston so as to compress the contents of a cylinder), or if work is done by the system, which changes its temperature (such as heating the gas in a cylinder to cause a piston to move). Шаблон:Mvar applies only if <math>P\,\mathrm{d}V = 0</math>, that is, no work is done. Consider the difference between adding heat to the gas with a locked piston and adding heat with a piston free to move, so that pressure remains constant.

In the second case, the gas will both heat and expand, causing the piston to do mechanical work on the atmosphere. The heat that is added to the gas goes only partly into heating the gas, while the rest is transformed into the mechanical work performed by the piston.

In the first, constant-volume case (locked piston), there is no external motion, and thus no mechanical work is done on the atmosphere; Шаблон:Mvar is used. In the second case, additional work is done as the volume changes, so the amount of heat required to raise the gas temperature (the specific heat capacity) is higher for this constant-pressure case.

Ideal-gas relations

For an ideal gas, the molar heat capacity is at most a function of temperature, since the internal energy is solely a function of temperature for a closed system, i.e., <math>U=U(n,T)</math>, where Шаблон:Mvar is the amount of substance in moles. In thermodynamic terms, this is a consequence of the fact that the internal pressure of an ideal gas vanishes.

Mayer's relation allows us to deduce the value of Шаблон:Mvar from the more easily measured (and more commonly tabulated) value of Шаблон:Mvar:

<math>C_V = C_P - nR.</math>

This relation may be used to show the heat capacities may be expressed in terms of the heat capacity ratio (Шаблон:Math) and the gas constant (Шаблон:Mvar):

<math>C_P = \frac{\gamma n R}{\gamma - 1} \quad \text{and} \quad C_V = \frac{n R}{\gamma - 1},</math>

Relation with degrees of freedom

The classical equipartition theorem predicts that the heat capacity ratio (Шаблон:Math) for an ideal gas can be related to the thermally accessible degrees of freedom (Шаблон:Mvar) of a molecule by

<math> \gamma = 1 + \frac{2}{f},\quad \text{or} \quad f = \frac{2}{\gamma - 1}.</math>

Thus we observe that for a monatomic gas, with 3 translational degrees of freedom per atom:

<math> \gamma = \frac{5}{3} = 1.6666\ldots,</math>

As an example of this behavior, at 273 K (0 °C) the noble gases He, Ne, and Ar all have nearly the same value of Шаблон:Math, equal to 1.664.

For a diatomic gas, often 5 degrees of freedom are assumed to contribute at room temperature since each molecule has 3 translational and 2 rotational degrees of freedom, and the single vibrational degree of freedom is often not included since vibrations are often not thermally active except at high temperatures, as predicted by quantum statistical mechanics. Thus we have

<math> \gamma = \frac{7}{5} = 1.4.</math>

For example, terrestrial air is primarily made up of diatomic gases (around 78% nitrogen, N₂, and 21% oxygen, O₂), and at standard conditions it can be considered to be an ideal gas. The above value of 1.4 is highly consistent with the measured adiabatic indices for dry air within a temperature range of 0–200 °C, exhibiting a deviation of only 0.2% (see tabulation above).

For a linear triatomic molecule such as Шаблон:CO2, there are only 5 degrees of freedom (3 translations and 2 rotations), assuming vibrational modes are not excited. However, as mass increases and the frequency of vibrational modes decreases, vibrational degrees of freedom start to enter into the equation at far lower temperatures than is typically the case for diatomic molecules. For example, it requires a far larger temperature to excite the single vibrational mode for Шаблон:Chem2, for which one quantum of vibration is a fairly large amount of energy, than for the bending or stretching vibrations of Шаблон:CO2.

For a non-linear triatomic gas, such as water vapor, which has 3 translational and 3 rotational degrees of freedom, this model predicts

<math> \gamma = \frac{8}{6} = 1.3333\ldots.</math>

Real-gas relations

As noted above, as temperature increases, higher-energy vibrational states become accessible to molecular gases, thus increasing the number of degrees of freedom and lowering Шаблон:Math. Conversely, as the temperature is lowered, rotational degrees of freedom may become unequally partitioned as well. As a result, both Шаблон:Mvar and Шаблон:Mvar increase with increasing temperature.

Despite this, if the density is fairly low and intermolecular forces are negligible, the two heat capacities may still continue to differ from each other by a fixed constant (as above, Шаблон:Math), which reflects the relatively constant Шаблон:Mvar difference in work done during expansion for constant pressure vs. constant volume conditions. Thus, the ratio of the two values, Шаблон:Math, decreases with increasing temperature.

However, when the gas density is sufficiently high and intermolecular forces are important, thermodynamic expressions may sometimes be used to accurately describe the relationship between the two heat capacities, as explained below. Unfortunately the situation can become considerably more complex if the temperature is sufficiently high for molecules to dissociate or carry out other chemical reactions, in which case thermodynamic expressions arising from simple equations of state may not be adequate.

Thermodynamic expressions

Values based on approximations (particularly Шаблон:Math) are in many cases not sufficiently accurate for practical engineering calculations, such as flow rates through pipes and valves at moderate to high pressures. An experimental value should be used rather than one based on this approximation, where possible. A rigorous value for the ratio Шаблон:Mvar can also be calculated by determining Шаблон:Mvar from the residual properties expressed as

<math> C_P - C_V = -T \frac{\left(\frac{\partial V}{\partial T}\right)_P^2}{\left(\frac{\partial V}{\partial P}\right)_T} = -T \frac{\left(\frac{\partial P}{\partial T}\right)_V^2}{\left(\frac{\partial P}{\partial V}\right)_T}.</math>

Values for Шаблон:Mvar are readily available and recorded, but values for Шаблон:Mvar need to be determined via relations such as these. See relations between specific heats for the derivation of the thermodynamic relations between the heat capacities.

The above definition is the approach used to develop rigorous expressions from equations of state (such as Peng–Robinson), which match experimental values so closely that there is little need to develop a database of ratios or Шаблон:Mvar values. Values can also be determined through finite-difference approximation.

Adiabatic process

Шаблон:See also This ratio gives the important relation for an isentropic (quasistatic, reversible, adiabatic process) process of a simple compressible calorically-perfect ideal gas:

<math>PV^\gamma</math> is constant

Using the ideal gas law, <math>PV = nRT</math>:

<math>P^{1-\gamma} T^\gamma</math> is constant

<math>TV^{\gamma-1}</math> is constant

where Шаблон:Mvar is the pressure of the gas, Шаблон:Mvar is the volume, and Шаблон:Mvar is the thermodynamic temperature.

In gas dynamics we are interested in the local relations between pressure, density and temperature, rather than considering a fixed quantity of gas. By considering the density <math>\rho = M/V</math> as the inverse of the volume for a unit mass, we can take <math>\rho = 1/V</math> in these relations. Since for constant entropy, <math>S</math>, we have <math>P \propto \rho^\gamma</math>, or <math> \ln P = \gamma \ln \rho + \mathrm{constant}</math>, it follows that

<math> \gamma = \left.\frac{\partial \ln P}{\partial \ln \rho}\right|_{S}.</math>

For an imperfect or non-ideal gas, Chandrasekhar defined three different adiabatic indices so that the adiabatic relations can be written in the same form as above; these are used in the theory of stellar structure:

<math>\begin{align}

                      \Gamma_1 &= \left.\frac{\partial \ln P}{\partial \ln \rho}\right|_{S}, \\[2pt]
 \frac{\Gamma_2 - 1}{\Gamma_2} &= \left.\frac{\partial \ln T}{\partial \ln P}\right|_{S}, \\[2pt]
                  \Gamma_3 - 1 &= \left.\frac{\partial \ln T}{\partial \ln \rho}\right|_{S}.

\end{align}</math>

All of these are equal to <math>\gamma</math> in the case of an ideal gas.

See also

• Relations between heat capacities
• Heat capacity
• Specific heat capacity
• Speed of sound
• Thermodynamic equations
• Thermodynamics
• Volumetric heat capacity