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Question

For real gases the relation between, P, V and T is given by van der Waals' equation

(P+an2V2)(Vnb)=nRT

where 'a' and 'b' are van der Waals' constants, 'nb' is approximately equal to the total volume of the molecules of a gas. 'a' is the measure of the magnitude of intermolecular attraction.

(i) Arrange the following gases in the increasing order of 'b' Give reason.

O2, CO2, H2, He

(ii) Arrange the following gases in the descending order of magnitude of 'a'. Give reason.

CH4, O2, H2

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Solution

(i) The molar volume occupied by the gas molecules size of the molecules and van der Waals' constant 'b' represents the molar volume of the gas molecules. Hence, the value of 'b' increases in the following order

H2 < He < O2 < CO2

(ii) van der Waals' constant 'a' is the measure of the magnitude of intermolecular attraction. The magnitude of intermolecular increases with increase in the size of the electron cloud in a molecule. Hence, for the given gases magnitude of 'a' decreases in the following order

CH4 > O2 > H2

Greater the size of the electron cloud, greater is the polarisability of the molecule and greater is the dispersion forces or London forces.


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