This preview shows pages 1–4. Sign up to view the full content.
Chapter 19
The Kinetic Theory of Gases
1
PHYS 2101, P.M.Shikhaliev
LSU,
Fall 2010
This preview has intentionally blurred sections. Sign up to view the full version.
View Full Document 19.2. Avogadro’s Number
Avogadro’s number and “mole” quantity:
Let us we have two gas samples: 1
st

N
molecules of
H
2
, and 2
nd

N
molecules of
O
2
The mass of the
H
2
sample is M
H
= (N)x(2amu) = (N)x(2)x(1.66 x10
24
g)
The mass of
the
O
2
sample is N
O
= (N)x(32amu) = (N)x(32)x(1.66 x10
24
g)
If we select
N = 6.02 x 10
23
, then (N)x(1.66 x10
24
g) = 1 g, and
M
H
= 2 g, and M
O
= 32 g
The number
N
A
= N = 6.02 x 10
23
is called
Avogadro’s
number
By convention,
Avogadro’s
number is defined as number of atoms in
12 g
Carbon.
The amount of matter including
N
A
atoms is called
1 mole
of this matter
All gases including
N
A
atoms or molecules have same volume of
V
A
= 22.4 L
Molar mass
M = N
A
x m
, where
m
is the mass of the atom or molecule
2
PHYS 2101, P.M.Shikhaliev
LSU,
Fall 2010
Avogadro’s Law:
All gases having
same
volume,
same
pressure, and
same
temperature
contain
same
numbers of molecules.
19.3. Ideal Gases
Here
p
is the absolute pressure,
n
is the number of moles of gas present, and
T
is
its temperature in Kelvin's.
R
is the gas constant that has the same value for all
gases.
3
This preview has intentionally blurred sections. Sign up to view the full version.
View Full Document
This is the end of the preview. Sign up
to
access the rest of the document.
This note was uploaded on 01/26/2011 for the course PHYS 2101 taught by Professor Grouptest during the Spring '07 term at LSU.
 Spring '07
 GROUPTEST
 Physics

Click to edit the document details