# Molar Volume - PowerPoint

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```					Molar Volume
Chemistry
Pressure
• Gas pressure is a result of gas particles colliding
with the walls of a container
• The unit for pressure is the pascal (Pa) and is
equal to 1N/m2
• Normally pressure is reported in kilopascals
(kPa) which is 1000Pa
• A non-rigid container (i.e. balloon) will change
volume so that the atmospheric pressure outside
the container is the same as the pressure inside
the container
Charles’s Law
• Explains the
relationship between
volume and
temperature (if         V1 V2
pressure is held
constant)

• States that the ratio   T1 T2
between volume and
temperature will be
constant
Boyle’s Law
• Explains the
relationship between
volume and pressure
(if temperature is held
constant)
p1V1  p2V2
• States that the
product of pressure
and volume will be
constant
Ideal Gas Law
• Combines Charles’s
and Boyle’s Law
along with the mole
concept to explain an
ideal gas                pV  nRT
• Involves the ideal gas
constant (R =
8.314472 JK-1mol-1)
Standard Temperature and
Pressure and Standard Ambient
Temperature and Pressure
• There are two standards that have been
established for temperature and pressure:
– STP – 273K and 101.3kPa
– SATP – 298K and 100kPa
• These will be crucial when dealing with the
concept of Molar Volume
Molar Volume
• For each of the gases on the periodic table
look up:
– Their density (g/L)
– Their molar mass (remember some are
diatomic) (g/mol)
• Then calculate:
– The volume one mole of gas would occupy
Molar Volume
• The two commonly used values for Molar
Volume are:
VSTP  22.4L / mol
VSATP  24.8L / mol
• The equation we will use to employ Molar
Volume is:
v
n
V
Practice Problems
• Page 73
– Questions 38-43

• Section Review
– Questions 1-6, Page 74

• Chapter Review
– Page 75-77

```
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