Molar Volume
MOLAR VOLUME
Note that gases are compressible. Compressibility can be adjusted by altering the pressure and temperature.
When one does that, you alter the amount of space it occupies, i.e. its volume.
Volume rather than mass is a better and more accurate way to determine the amount of gas and is a better dimension to work with.
There is also ROOM TEMPERATURE AND PRESSURE (r.t.p). This means implies a specific temperature and pressure of 293K and 1atm.
Gases at r.t.p occupy a volume of 24.0dm3 and gases at s.t.p occupy a volume of 22.4dm3.
This is for 1 mole of ANY gas.
NB: 1L=1dm3=1000cm3
Mass of HCl= 36.5g
Since we know any gas at s.t.p has a volume of 22.4 dm3 contains 1 mole.
THEN
If 22.4 dm3 of HCl has a mass of 36.5g at s.t.p
Then 44.8 dm3 of HCl has a mass of 36.5g x 44.8 dm3 / 22.4 dm3
Example 2:
How many molecules are present in 22.4 dm3 of SO2 at s.t.p?
If 22.4 dm3 SO2 contains 6.02 x1023
Then 2.24dm3 SO2 contains 6.02 x1023 x 2.24/22.4= 6x10 molecules.
- Set induction
Note that gases are compressible. Compressibility can be adjusted by altering the pressure and temperature.
When one does that, you alter the amount of space it occupies, i.e. its volume.
Volume rather than mass is a better and more accurate way to determine the amount of gas and is a better dimension to work with.
- WHAT YOU NEED TO KNOW!
There is also ROOM TEMPERATURE AND PRESSURE (r.t.p). This means implies a specific temperature and pressure of 293K and 1atm.
Gases at r.t.p occupy a volume of 24.0dm3 and gases at s.t.p occupy a volume of 22.4dm3.
This is for 1 mole of ANY gas.
NB: 1L=1dm3=1000cm3
- AVOGADRO’S LAW:
- Example 1:
Mass of HCl= 36.5g
Since we know any gas at s.t.p has a volume of 22.4 dm3 contains 1 mole.
THEN
If 22.4 dm3 of HCl has a mass of 36.5g at s.t.p
Then 44.8 dm3 of HCl has a mass of 36.5g x 44.8 dm3 / 22.4 dm3
Example 2:
How many molecules are present in 22.4 dm3 of SO2 at s.t.p?
If 22.4 dm3 SO2 contains 6.02 x1023
Then 2.24dm3 SO2 contains 6.02 x1023 x 2.24/22.4= 6x10 molecules.
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