Question

Henry's law constants for aqueous solution of $CO , O _{2}, CO _{2}$ and $C _{2} H _{2}$ gases are respectively at $25^{\circ} C$ as $58 \times 10^{3}, 43 \times 10^{3}, 1.61 \times 10^{3}$ and $1.34 \times 10^{3}$. The solubility of these gases decreases in the order

• A. $CO>O_{2}>CO_{2}>C_{2}H_{2}$
• B. $O_{2}>CO_{2}>CO>C_{2}H_{2}$
• C. $C_{2}H_{2}>CO_{2}>O_{2}>CO$
• D. $O_{2}>CO_{2}>C_{2}H_{2}>CO$

Answer 1

Answer: (C)

$C_{2}H_{2}>CO_{2}>O_{2}>CO$

Answer 2

$p=K_{H} X$; Higher the value of $K_{H}$ at a given pressure, the lower is the solubility of the gas in the liquid.
Therefore, the solubility of the given gases decreases in the order
$C _{2} H _{2}> CO _{2}> O _{2}> CO$