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Gas law

1. *Gas Laws*

2. Physical Characteristics of Gases
Physical Characteristics Typical Units
Volume, V liters (L)
Pressure, P atmosphere
(1 atm = 1.015x10
5
N/m
2
)
Temperature, T Kelvin (K)
Number of atoms or
molecules, n
mole (1 mol = 6.022x10
23

atoms or molecules)

3.  Pressure and volume
are inversely related at
constant temperature.
 PV = K
 As one goes up, the other
goes down.
 P
1
V
1
= P
2
V
2
Boyle’s Law
“Father of Modern Chemistry”
Robert Boyle
Chemist & Natural Philosopher
Listmore, Ireland
January 25, 1627 – December 30, 1690

4. Boyle’s Law: P
1
V
1
= P
2
V
2

5. Boyle’s Law: P
1
V
1
= P
2
V
2

6.  Volume of a gas varies
directly with the absolute
temperature at constant
pressure.
 V = KT
 V
1
/ T
1
= V
2
/ T
2
Charles’ Law
Jacques-Alexandre Charles
Mathematician, Physicist, Inventor
Beaugency, France
November 12, 1746 – April 7, 1823

7. Charles’ Law: V
1/T
1 = V
2/T
2

8. Charles’ Law: V
1/T
1 = V
2/T
2

9. At constant temperature
and pressure, the volume of
a gas is directly related to
the number of moles.
V = K n
V
1 / n
1 = V
2 / n
2
Avogadro’s Law
Amedeo Avogadro
Physicist
Turin, Italy
August 9, 1776 – July 9, 1856

10. Avogadro’s Law: V
1
/n
1
=V
2
/n
2

11.  At constant volume,
pressure and absolute
temperature are
directly related.
 P = k T
 P
1
/ T
1
= P
2
/ T
2
Gay-Lussac Law
Joseph-Louis Gay-Lussac
Experimentalist
Limoges, France
December 6, 1778 – May 9, 1850

12. The total pressure in a container
is the sum of the pressure each
gas would exert if it were alone
in the container.
The total pressure is the sum of
the partial pressures.
P
Total = P
1 + P
2 + P
3 + P
4 + P
5 ...
(For each gas P = nRT/V)
Dalton’s Law
John Dalton
Chemist & Physicist
Eaglesfield, Cumberland, England
September 6, 1766 – July 27, 1844

13. Dalton’s Law

14. Water evaporates!
When that water evaporates, the vapor has a
pressure.
Gases are often collected over water so the vapor
pressure of water must be subtracted from the
total pressure.
Vapor Pressure

15. Differences Between Ideal and Real Gases
Obey PV=nRT AlwaysOnly at very low
P and high T
Molecular volume Zero Small but
nonzero
Molecular attractionsZero Small
Molecular repulsionsZero Small
Ideal Gas Real Gas

16. Real molecules do take up space and do interact
with each other (especially polar molecules).
Need to add correction factors to the ideal gas
law to account for these.
Real Gases

17. 
[P
obsa (
n
V
)
2
] (Vnb)nRT
Corrected PressureCorrected Volume
Van der Waal’s equation
 “a” and “b” are
determined by experiment
 “a” and “b” are
different for each gas
 bigger molecules have larger “b”
 “a” depends on both
size and polarity
Johannes Diderik van der Waals
Mathematician & Physicist
Leyden, The Netherlands
November 23, 1837 – March 8, 1923

18. 18
Kinetic Molecular Theory of Gases
1.A gas is composed of molecules that are separated from
each other by distances far greater than their own
dimensions. The molecules can be considered to be points;
that is, they possess mass but have negligible volume.
2.Gas molecules are in constant motion in random directions,
and they frequently collide with one another. Collisions
among molecules are perfectly elastic.
3.Gas molecules exert neither attractive nor repulsive forces
on one another.
4.The average kinetic energy of the molecules is proportional
to the temperature of the gas in kelvins. Any two gases at
the same temperature will have the same average kinetic
energy
KE = 3/2 RTKE = ½ mu
2