Henry's constant (in kbar) for four gases $α, β, γ$ and $δ$ in water at $298 K$ is given below :
$\begin{matrix} α & β & γ & δ \\ K_{H} & 50 & 2 & 2 \times 10^{- 5} & 0.5 \end{matrix}$
(density of water $= 10^{3} k {gm}^{- 3}$ at $298 K$ ) This table implies that :

Question

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

$\begin{matrix} α & β & γ & δ \\ K_{H} & 50 & 2 & 2 \times 10^{- 5} & 0.5 \end{matrix}$

(density of water $= 10^{3} k {gm}^{- 3}$ at $298 K$ ) This table implies that :

TestHub · Accepted Answer

(1) From Henery's law P = k H X Higher the value of k H smaller will be solubility so γ is more soluble. (2) Though solubility of gas will decrease with increase in temperature but this conclusion can not be drawn from the given table. (3)For δ ⇒ P δ = K Hδ . X δ = 0 . 5 × 10 3 × 55 . 55 55 . 55 + 1000 18 = 250 bar . (4)For γ p γ = K H γ × x γ = 2 × 10 - 2 55 . 5 55 . 5 + 1000 18 = 10 - 2 bar

Chemistry - Liquid Solution Question with Solution | TestHub

Options:

Doubts & Discussion