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प्रश्न
For real gases the relation between p, V and T is given by van der Waals equation:
`p + (an^2)/V^2 (V - nb) = 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 magnitude of intermolecular attraction.
Arrange the following gases in the decreasing order of magnitude of ‘a’. Give reason.
\[\ce{CH4, O2, H2}\]
उत्तर
The decreasing order of magnitude of ‘a’ of the given molecule is \[\ce{CH4 > O2 > H2}\]
The Van der waals constant ‘a’ represents the magnitude of intermolecular attraction which increases with increase in the size of the electron cloud of the molecule. So the greater the size of a molecule, greater will be the electron cloud and hence greater will be the polarisability and more will be the magnitude of intermolecular attraction.
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संबंधित प्रश्न
What will be the minimum pressure required to compress 500 dm3 of air at 1 bar to 200 dm3 at 30°C?
What would be the SI unit for the quantity pV2T 2/n?
For real gases the relation between p, V and T is given by van der Waals equation:
`p + (an^2)/V^2 (V - nb) = 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 magnitude of intermolecular attraction.
Arrange the following gases in the increasing order of ‘b’. Give reason.
\[\ce{O2, CO2, H2, He}\]
