Four vessels of same volume consist equal moles of four gases H ₂, Cl ₂ , N ₂ and O ₂ separately at same temperature. The pressure exerted by the gas is maximum for -

Step-by-step solution

The gases demonstrate real behavior where pressure deviates from the ideal gas law due to intermolecular forces and molecular volume. The van der Waals equation P = nRT V - nb - an^2 V^2 governs this behavior, with a representing intermolecular attraction and b representing excluded volume. For fixed n , V , and T , the compressibility factor Z = PV nRT approximates to Z 1 + n V (b - a RT ) , making pressure maximization equivalent to maximizing (b - a RT ) . At T = 300 K, using standard van der Waals constants: H