The gas Laws
1.
Boyle's Law
The volume of a given mass of gas at constant temperature is inversely
proportional to its pressure, i.e.
Pv = K
where, P is the pressure and v is the volume of
a fixed quantity of gas at constant temperature, k is the constant.
2. Charle's Law
At constant pressure the volume of a given mass of any gas is proportional to
its temperature on the absolute scale. It is the temperature on the
centigrade scale, then the absolute temperature T (k) is equal to t + 273.
Therefore Charles Law can be expressed as:-
V = k (t + 273)
V = KT.
Boyle's and Charle's Law can now be combined to
give the following relationship.
Pv = RT or Pv/T = k
The absolute temperature (kelvin) scale is as mentioned above, obtained by
adding 273 to the temperature in degrees celsius.
For example
20 degree C = (20 +
273) = 293 k.
-10 degree C = (-10 + 273) = 263
k.
3. Avogadro's
Law
Equal volumes of all gases at the same temperature and pressure contain equal
numbers of molecules. One gram mole of any gas at a given temperature and
pressure will therefore occupy a definite volume, which will be the same for all
gases. Therefore the value R in the equation PV = RT will also be the same
for all gases. This standard value is usually indicated by a special
symbol R, the gas constant.
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