Practicing Success
Passage: Solubility of gases in liquids is greatly affected by pressure and temperature. Henry gave the quantitative relationship between pressure and solubility of gas in a solvent. According to Henry’s law, partial pressure of a gas above a liquid is directly proportional to its mole fraction in solution and is expressed as \(P = K_H.x\), where \(K_H\) is Henry’s constant and x is mole fraction of gas. \(K_H\) is a function of nature of gas. F M Raoult gave a quantitative relationship between partial pressures and mole fractions in the binary solution of volatile liquids. Raoult’s law states that for a binary solution of volatile liquids, the partial pressure of each component in the solution is directly proportional to its mole fraction. Thus for a solution of component \(1\) and \(2\), partial pressure of each component\(P_1 = p_1^0x_1\), where \(p_1^0\) is the vapour pressure of pure component \(1\) at the same temperature. Similarly \(P_2 = p_2^0x_2\) |
Solubility of Carbon dioxide in soda water increases with |
Increase in pressure and temperature both Increase in pressure and decrease in temperature Decrease in pressure and increase in temperature Decrease in pressure and decrease in temperature |
Increase in pressure and decrease in temperature |
The correct answer is option 2. Increase in pressure and decrease in temperature. The solubility of gases in liquids is influenced by both pressure and temperature, and Henry's Law describes this relationship. Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. In the case of carbon dioxide \((CO_2)\) dissolving in soda water, the relationship between solubility and pressure and temperature can be explained as follows: 1. Pressure Effects: 2. Temperature Effects: |