Question

Match gases under specified conditions listed in Column 1 with their properties/laws in Column II.

$$\begin{array}{cccc}& ColumnI& & ColumnII\\ A& Hydrogengas⟮p=200atm,T=273K⟯& p& Compressionfactor=1\\ B& Hydrogengas⟮p=0atm,T=273K⟯& q& Attractiveforcesaredominant\\ C& C{O}_2⟮p=1atm,T=273K⟯& r& pV=nRT\\ D& Realgaswithverylargemolarvolume& s& p⟮V-nb⟯=nRT\end{array}$$

• A. A →(r), B →(p), C →(s), D →(q)
• B. A →(p,s), B →(r), C →(p,q), D →(p,s)
• C. A →(q), B →(p), C →(s), D →(r)
• D. A →(p), B →(q), C →(r), D →(s)

Answer 1

The correct option is B

A →(p,s), B →(r), C →(p,q), D →(p,s)

A $\to$ (p, s); B $\to$ (r); C $\to$ (p, q); D $\to$ (p, s)

(A) Z = 1 for ideal gas. At low temperature and high pressure, real gases show ideal behaviour which means the equation [$p+\frac{a{n}^2}{V^2}$][V - nb] = nRT reduces to p(V - nb) = nRT.

(B) For $H_2$ gas, the value of Z = 1 at p = 0 and it increases continuously on increasing p

(C) $C{O}_2$ molecules have larger attractive forces, under normal conditions.

(D) As Z = $\frac{p{V}_m}{RT}$, at very large molar volume Z is not equal to 1.