Question

Henry's constant (in k bar) for four gases α, β, γ and δ in water at 298 K is given below:

	α	β	γ	δ
KH	50	2	2 × 10-5	0.5

(density of water = 10³ kg m^-3 at 298 K)

This table implies that:

पर्याय

• α a has the highest solubility in water at a given pressure 

• solubility of γ at 308 K is lower than at 298 K 

• The pressure of 55.5 molal solution of γ is 1 bar

• The pressure of a 55.5 molal solution of δ is 250 bar

Answer 1

The pressure of a 55.5 molal solution of δ is 250 bar

Explanation:

(a) From Henry's law p = K_H(x)

Higher the value of K_H, smaller will be the solubility of the gas, soy is more soluble.

(b) Though solubility of gases will decrease with increase in temperature but this conclusion can not be drawn from the given table.

(c) For γ

`("p")_gamma = ("K"_"H")_gamma * (x)_gamma`

`= 2 xx 10^-5 [55.5/(55.5 + 1000/18)]`

`= 10^-5` k bar = 10^-2 bar

(d) For δ

`("p")_δ = ("K"_"H")_δ * (x)_δ`

`= 0.5 [55.5/(55.5 + 1000/18)]`

`= 0.5 xx 0.5 = 0.25` k bar = 250 bar