At constant temperature, two gases A and B are dissolved separately in the same liquid under the same pressure. If $K_H(A) > K_H(B)$, which statement is correct?
AGas A is more soluble than gas B
BGas B is more soluble than gas A
CBoth gases have equal solubility
DSolubility cannot be compared from $K_H$ values
Answer & Solution
Correct answer: B. Gas B is more soluble than gas A
For Henry's law written as $P = K_H x$, at the same pressure $x = P/K_H$. Therefore the gas with smaller $K_H$ has larger mole fraction in solution and is more soluble. So B is more soluble than A.
Related questions
The nitric acid and water azeotrope holds nitric acid at about:Distilling an ethanol and water mixture stops at about:A large negative deviation produces an azeotrope that is:A large positive deviation produces an azeotrope that is:The components of an azeotrope cannot be separated by:Binary mixtures boiling at a constant temperature are called:Chloroform and acetone form a hydrogen bond, so the vapour pressure:A mixture of phenol and aniline shows: