DOC.
4
KINETIC THEORY LECTURE NOTES
179
universal constant
•
absolute
temperature.
We
will delve
into
this
later
on,
when
discussing
the
second
law.
At the
present
we
will
proceed
in
the
following
way.[64]
We
will conceive
of the absolute
temperature
as
defined
with
the
aid
of
ideal
gases by
the
equation
of
state
pV
=
RT
We
have
just
found
from kinetics
that
pV=NB
By
comparing
the
right-hand
sides
0
=
-T
N
Thus,
8
is
equal
to
the absolute
temperature multiplied
by
a
(numerically very small)
constant
(about 1.4
10-16).
We
can
also calculate the
most
common mean
values
of
the
velocity
of
gas
molecules
[p. 32]
_
(V
+
n2
+
C2)
dW
=
const
e
m
d£dx\dt
How
large
is
the
probability
of
c
being
between
c
&
c +
dc?
Integrate
over
the
spherical
shell
_e
dWdc
=
cons
e
m c2dc
we
thus obtain