Question

Henry's constant (in kbar) for four gases $\alpha, \beta$, $\gamma$ and $\delta$ in water at $298 K$ is given below:

	$\alpha$	$\beta$	$\gamma$	$\delta$
$K_H$	$50$	$2$	$2 \times 10^{-5}$	$0.5$

(density of water $=10^{3} kg m ^{-3}$ at $\left.298 K \right)$ This table implies that :

• A. The pressure of a 55.5 molal solution of $\gamma$ is 1 bar
• B. The pressure of a 55.5 molal solution of $\delta$ is 250 bar
• C. Solubility of $\gamma$ at $308 K$ is lower than at $298 K$
• D. $\alpha$ has the highest solubility in water at a given pressure

Answer 1

Answer: (C)

(1) $P _{\gamma}= K _{ H } X _{ Y }$

$P _{\gamma}= 2 \times 10^{-15} \times \frac{55.5}{55.5+\frac{1000}{18}}$

$=2 \times 10^{-5} K$ bar

$=2 \times 10^{-2}$ bar

(2) $P _{\delta}= K _{ H } X _{8}$

$P _{\delta}=0.5 \times \frac{55.5}{55.5+\frac{1000}{18}}=.249 K$ bar $=249$ bar

(3) On increasing temperature solubility of gases decreases

(4) $K _{ H } \downarrow$ solubility $\uparrow$ and lowest $K _{ H }$ is for $\gamma$