Match gases under specified condition listed in Column I with their proerties/laws in Column II.

Answer

`A rarr p , s; B rarr r; C rarr p,q; D rarr r`

Explanation

(A) Explanation `:` Vander Waals' equation
For hydrogen gas `(P = 200 atm, T= 273 K)`
As pressure is large, `V_(m)` can be assumed small, thus 'b' can not be ignored, while due to high pressure , `a// V_(m)^(2)` can be considered negligible in comparison to P.
Hence, equation gets reduced to
`P(V_(m)-b)= RT` and `Z = 1+(Pb)/(RT) P(V_(m)-b)= RT` and `Z = 1+(Pb)/(RT)`
(b) For hydrogen gas `(P-0,T=273K)`
when pressure occurs of low order about 1 atm or less and temperature is not very close to the point of liquefaction `[T_(c ) (H_(2))= 33.3K]` gas behaves ideally
`PV = nRT`
(C ) For `CO_(2)(P =1 atm , T= 273K)`
Temperature is close to the point of liquefaction `[T_(c) (CO_(2))= 304.2)` thus, deviation from ideality appears very high ( due to high attractive force of attraction ).
(D ) For real gas with very large molar volume.
As molar volume is very large , `a//V_(m)^(2)` will be negligible and at the same time 'b' in comparison to `V_(m)` is also considered negligible , thus, `PV_(m) =nRT`