The «temperature» of a gas (if you must use a compound term) is a measure of
the total kinetic energy of the molecules in the volume of gas being measured.
Not exact matches
The
kinetic energy of the in the the
molecules at the top
of the box and the
molecules at the bottom
of the box are different, in the additive fashion
of kinetic energy plus potential
energy equals a constant
total energy.
Over a sufficiently long period
of time, it follows from the equipartition theorem and other principles
of statistical mechanics that every
molecule in a gas will have the same average
kinetic energy, the same average potential
energy, and the same
total energy, as any other
molecule.
For Velasco et al.'s purposes, the state
of a
molecule is totally defined by its location and momentum, and the state
of an ensemble
of molecules is the combination
of the individual
molecules» states: for an ideal - gas ensemble consisting
of N monatomic
molecules, each
of which is characterized by x, y, and z components both
of position and
of momentum, the ensemble's state can be represented by a point in 6N space, in which a surface I think
of as a hyperparaboloid represents the states that exhibit a given
total (potential +
kinetic)
energy.
The individual
molecules in the upper atmosphere can indeed be very hot (high
kinetic energy), but there are so few
of them, their
total temperature on any thermometer is very low.
This must drop the temperature
of the
molecules in question, since temperature is only a measure
of the
KINETIC ENERGY side
of the
TOTAL ENERGY equation.
If you read Velasco et al.'s Equation 8 for mean single -
molecule kinetic energy K as a function
of altitude z, you'll see that the expression for K is the product
of a constant and (1 - mgz / E), where m is molecular mass, g is the acceleration
of gravity, and E is
total system
energy.
Does he mean the individual the temperature
of individual
molecules (molecular
kinetic energy), or does he mean the temperature
of the
total airmass?