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Hydrogen always shows positive deviation...

Hydrogen always shows positive deviation in the compressibility factor vs pressure curves . Why ?

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Hydrogen molecules have small size. Intermolecular repulsions operate between molecules of hydrogen.
The real volume of hydrogen gas is more than the ideal volume
Hence, z `gt` 1 for hydrogen at any pressure.
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At a particular temperature and pressure for a real gas Van der Waal's equation can be written as: (P + a/(V^(2)m)) (V_(m) -b) =RT where Vm is molar volume of gas. This is cubic equation in the variable Vm and therefore for any single value of P & T there should be 3 values of Vm. Which are shown in graph as Q, M and L. As temperature is made to increase at a certain higher temperature the three values of Vm becomes identical. The temperature, pressure & molar volume at point X are called Tc, Pc & Vc for real gas. The compressibility factor in terms of Pc, Vc and T is called Zc. The value of critical compressibility factor Zc is approximately

At a particular temperature and pressure for a real gas Van der Waal's equation can be written as: (P + a/(V^(2)m)) (V_(m) -b) =RT where Vm is molar volume of gas. This is cubic equation in the variable Vm and therefore for any single value of P & T there should be 3 values of Vm. Which are shown in graph as Q, M and L. As temperature is made to increase at a certain higher temperature the three values of Vm becomes identical. The temperature, pressure & molar volume at point X are called Tc, Pc & Vc for real gas. The compressibility factor in terms of Pc, Vc and T is called Zc. The expression of Van dcr Waal's constant 'a' can be given as

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