Henry’s constant (in kbar) for four gases $\alpha $, $\beta $, $\gamma $ and $\delta $ in water at 298 K is given below : .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-baqh{text-align:center;vertical-align:top} $\alpha $ $\beta $ $\gamma $ $\delta $ KH 50 2 2 $ \times $ 10-5 0.5 (density of water = 103 kg m-3 at 298 K) This table implies that :

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 = 10³ kg m^-3 at 298 K)
This table implies that :

solubility of $\gamma $ at 308 K is lower than at 298 K

The pressure of a 55.5 molal solution of $\delta $ is 250 bar

$\alpha $ has the highest solubility in water at a given pressure

The pressure of a 55.5 molal solution of $\gamma $ is 1 bar

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