Explanation
For positive deviation: PV = nRT + nPb. Thus, the factor nPb is responsible for increasing the PV value above ideal value. b is actually the effective volume of molecule. So, it is the finite size of molecules that leads to the origin of b and hence positive deviation at high pressure.
From Boyle’s law, pV = constant. Graph 3 represents a Boyle plot at a very low pressure.
υ = 0.921 u. Hence u : υ = 1.086 : 1.
Gases deviate form ideal behaviour because of intermolecular forces of attraction.
R = 0.0821 lit atm/degree/mole
Average kinetic energy depends only on temperature and does notdepend upon the nature of the gas.
At constant temp., the K.E. of the molecules remains the same
R ≠ 8.31 atm K-1 mol-1
‘a’ is directly related to forces of attraction. Hence greater the value of ‘a’,more easily the gas is liquefied.
In a closed flask, on heating the no. of moles does not change.
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