Gases Chemistry Worksheet - Chapter 13, An Introduction To Chemistry Page 28
ADVERTISEMENT
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
37
38
39
40
41
42
43
44
45
46
47
48
49510
Chapter 13
Gases
Table 13.1
Gases in Dry Air at STP
Gas
Percentage of total particles
Partial pressure (kPa)
nitrogen
78.081
79.116
oxygen
20.948
21.226
argon
0.934
0.995
carbon dioxide
0.035
0.035
neon
0.002
0.002
helium
0.0005
0.0005
methane
0.0001
0.0001
krypton
0.0001
0.0001
nitrous oxide
0.00005
0.00005
hydrogen
0.00005
0.00005
ozone
0.000007
0.000007
xenon
0.000009
0.000009
To get an understanding of the relationship between the total pressure of a mixture
O
20
bjeCtive
of gases and the partial pressure of each gas in the mixture, let’s picture a luminous
tube being filled with neon and argon gases. Let’s say the neon gas is added to the tube
first, and let’s picture ourselves riding on one of the neon atoms. The particle is moving
rapidly, colliding constantly with other particles and with the walls of the container.
Each collision with a wall exerts a small force pushing out against the wall. The total
pressure (force per unit area) due to the collisions of all of the neon atoms with the
walls is determined by the rate of collision of the neon atoms with the walls and the
average force per collision. The only ways that the neon gas pressure can be changed are
either by a change in the rate of collisions with the walls or by a change in the average
force per collision.
Now consider the effect on gas pressure of the addition of argon gas—at the same
temperature—to the tube that already contains neon. Assuming that the mixture of
gases acts as an ideal gas, there are no significant attractions or repulsions between the
particles, and the volume occupied by the particles is very small. Except for collisions
between particles, each gas particle acts independently of all of the other particles in
the tube. Now that there are also a certain number of argon atoms in the tube, the neon
atoms, including the one we are riding on, have more collisions with other particles
and change their direction of motion more often, but they still collide with the walls
at the same rate as before. If the temperature stays the same, the average velocity of the
neon atoms and their average force per collision with the walls is the same.
If the neon atoms in the mixture are colliding with the walls of the tube at the same
rate and with the same average force per collision as they did when alone, they are
exerting the same pressure against the walls now as they did when alone. Therefore,
the partial pressure of neon in the argon-neon mixture is the same as the pressure that
the neon exerted when it was alone. Assuming ideal gas character, the partial pressure
of any gas in a mixture is the pressure that the gas would exert if it were alone in the
container.
ADVERTISEMENT
0 votes
Related Articles
Related forms
Lines Worksheet - Chapter 1 An Introduction To Graphs And Lines, Math 1310 College Algebra, University Of Houston
Education
Chapter 2 An Introduction To Chemistry - The Structure Of Matter And The Chemical Elements Worksheet
Education
Notice, Chapter 13 Plan, Motions To Value Security, Avoid Judicial Lien, Avoid A Nonpurchase-money, Nonpossessory Security Interest And Lien, And/or To Assume Or Reject An Executory Contract/unexpired Lease
Legal
Order Dismissing Chapter 13 Case Prior To Confirmation Of Plan - United States Bankruptcy Judge
Financial
Related Categories
Parent category: Education