Adiabatic process
Adiabatic processes are processes in which no
heat is gained or lost in the working fluid. The term "adiabatic" describes things that are impermeable to heat transfer; for example, an adiabatic boundary is a boundary that is impermeable to heat transfer. An insulated wall approximates an adiabatic boundary condition.
Another example is the adiabatic flame temperature, which is the temperature that would be achieved by a flame in the absence of heat loss to the surroundings.
An adiabatic process which is also reversible is called an
isentropic process.
The opposite extreme, in which the maximum heat transfer with its surroundings occurs, causing the temperature to remain constant, is known as an isothermal process.
Adiabatic heating and cooling are processes that commonly occur due to a change in the pressure of a gas. This can be quantified using the ideal gas law.
There are three rates of adiabatic cooling for air.
 The ambient atmosphere lapse rate, which is the rate that air cools as one goes up in altitude.
 The dry adiabatic lapse rate, 10°C per 1000m rise.
 The wet adiabatic lapse rate, about 6° per 1000m rise.
The first rate is used to describe the temperature of the surrounding air that the rising air is passing through, and the second and third rates are in reference to a parcel of air that is rising through the atmosphere. The dry adabatic lapse rate applies to air which is below its
dew point, ie which is not saturated by
water vapor, whereas the wet adabatic lapse rate applies to air which has reached its dew point. Adabatic cooling is a common cause of
cloud formation.
Adiabatic cooling does not have to involve a fluid. One technique used to reach very low temperatures (thousandths and even millionths of a degree above absolute zero) is adiabatic demagnetisation, where the change in magnetic field on a magnetic material is used to provide adiabatic cooling.
The mathematical equation for an adiabatic process is

where P is pressure, V is volume, and

being the molar specific heat for constant pressure and
being the molar specific heat for constant volume.
For a monatomic ideal gas, .
Derivation of Formula
When heat transfer to the system is zero, .
Then, according to the first law of thermodynamics,

where
E is the internal energy of the system and
W is work done
by the system. Any work (W) done must be done at the expense of
internal energy E, since no heat Q is being supplied from the surroundings.
Pressurevolume work W done
by the system is defined as

However,
P does not remain constant during an adiabatic process but
instead changes along with
V.
It is desired to know how the values of and
relate to each other as the adiabatic process proceeds.
It will now be assumed that the system is a monatomic gas, so that

where
R is the universal gas constant.
Given and then
and
Now plug equations (2) and (3) into equation (1) to obtain

simplify,

divide both sides by
PV,

From the differential calculus it is then known that

which can be expressed as

for certain constants and of the
initial state. Then


Exponentiate both sides,

eliminate the minus sign,

therefore

and

Graphing Adiabats
Properties of adiabats on a PV diagram are:
(1) every adiabat asymptotically approaches both the V axis and the P axis (just like isotherms).
(2) each adiabat intersects each isotherm exactly once.
(3) an adiabat looks similar to an isotherm, except that during an expansion, an adiabat loses more pressure than an isotherm, so it has a steeper inclination (more vertical).
(4) if isotherms are concave towards the "northeast" direction (45 °), then adiabats are concave towards the "east northeast" (31 °).
(5) If adiabats and isotherms are graphed severally at regular changes of entropy and temperature, respectively (like altitude on a contour map), then as the eye moves outwards away from the axes (towards the northeast), it sees the density of isotherms stay constant, but it sees the density of adiabats drop. The exception is very near absolute zero, where the density of adiabats drops sharply and they become rare (see Nernst's theorem).
The following diagram is a PV diagram with a superposition of adiabats and isotherms:
The isotherms are the red curves and the adiabats are the black curves. The adiabats are isentropic. Volume is the abscissa and pressure is the ordinate.
In quantum mechanics, an adiabatic change is a sufficiently slow change in the
Hamiltonian which would result only in a change of eigenvalues, not eigenstates. Hence, if a system starts in the ground state, it will remain in the ground state of the system during the change, despite the fact that the properties of the ground state may change. If, in such a process, there is a qualitative change in the properties of the ground state (for example the
spin), the change is called a quantum phase transition.
See also: isothermal process, entropy, isochoric process, isobaric process, cyclic process.