To solve this problem, we need to understand the relationship between Henry's law constant $(K_H)$ and the solubility of gases in water.$\\$According to Henry's law, the solubility of a gas in a liquid is inversely proportional to the Henry's law constant $(K_H). \\$This means that a lower $K_H$ value indicates higher solubility of the gas in water.$\\$Given:$\\$• $K_H$ for gas A is $145$ kbar$\\$• $K_H$ for gas B is $2 \times 10^{-5}$ kbar$\\$• $K_H$ for gas C is $35$ kbar$\\$Let's compare the $K_H$ values:$\\$• Gas B has the smallest $K_H$ value, indicating it is the most soluble.$\\$• Gas C has the next smallest $K_H$ value, indicating it is more soluble than gas A but less soluble than gas B.$\\$• Gas A has the largest $K_H$ value, indicating it is the least soluble.$\\$Therefore, the order of solubility of these gases in water is:$\\$B > C > A$\\$This corresponds to Option 4.