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Match column-I with column-II : {:((A)...

Match column-I with column-II :
`{:((A)" Real gas at high pressure",(p)PV=RT+Pb),((B)" Force of attraction among gas Molecules is negligible",(q)PV=nRT),((C)" At high temp. and low pressure",(r)Z=1),((D)" Real gas at NTP",(s) (P+(an^(2))/(V^(2)))(V-nb)=nRT):}`

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`A rarr (p), B rarr (q), C rarr (q,r), D rarr (s)`
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The van der Waal equation of gas is (P + (n^(2)a)/(V^(2))) (V - nb) = nRT

The unit of the van der Waals gas equation parameter 'a' in (P+(an^(2))/(V^(2)))(V-nb)=nRT is :

{:(,"List-I(Van der Waals equation)",,"List-II(given by)"),("(a)","high pressure and low temperature",,"(p)PV=RT+Pb"),("(b)","low pressure",,(q)PV=RT-a//V),("(c)","Force of attraction is negligible",,"(r)PV=RT+aV"),("(d)","volume of molecule is negligible",,"(s)[P+a/V^(2)](V-b)=RT):}

{:(,"Column-I",,"Column-II"),("(P)","If volume of gas molecules be negligible",,(1)(P+a/V_(2))(V-b)=RT),("(Q)","At very high pressure",,"(2)PV=RT+Pb"),("(R)","At low pressure and high temperature",,(3)PV=RT-a/V),("(S)","van der Waal's gas",,"(4)PV=RT"):}

Real gases obey the gas equation : PV=nRT more correctly at low temperature and high pressure.

Assertion (A) : At high pressure , for one mole of a real gas , the compression factor Z is (1 + (Pb)/(RT)) Reason (R) : At high pressure , for one mole of a real gas , vanderwall equation is modified as P(V-b) = RT

Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is Z=(pV)/(nRT) The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at 0^(@)C and 100 atm pressure is found to be 0.5. The van der Waals gas equation is (p(an^(2))/(V^(2)))(V-nb)=nRT Calculate the value of 'a' assuming volume of molecules to be negligible.

Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is Z=(pV)/(nRT) The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at 0^(@)C and 100 atm pressure is found to be 0.5. The van der Waals gas equation is (p(an^(2))/(V^(2)))(V-nb)=nRT What is the value of Z for an ideal gas?

Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is Z=(pV)/(nRT) The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at 0^(@)C and 100 atm pressure is found to be 0.5. The van der Waals gas equation is (p(an^(2))/(V^(2)))(V-nb)=nRT What is the volume of the gas?