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Henry's constant (in kbar) for four gases α, β, γ and δ in water at 298 K is given below : K_H: α = 50, β = 2, γ = 2 × 10^-5, δ = 0.5 (density of water = 10^3 kg m^-3 at 298 K) This implies that -

1. α has the highest solubility in water at a given pressure
2. solubility of γ at 308 K is lower than at 298 K
3. The pressure of a 55.5 molal solution of γ is 1 bar
4. The pressure of a 55.5 molal solution of δ is 250 bar

Correct answer: The pressure of a 55.5 molal solution of γ is 1 bar

Solution

The correct option is accurate because Henry's law states that the solubility of a gas in a liquid is directly proportional to the pressure of that gas above the liquid. Given that γ has a very low Henry's constant, the pressure exerted by a 55.5 molal solution of γ would be approximately 1 bar, aligning with the relationship defined by Henry's law.

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