ANS:A - partial pressure of a component over a solution is proportional to its mole fraction in the liquid.

Henry's law states that the partial pressure of a component over a solution is proportional to its mole fraction in the vapour. Explanation:

• Henry's law describes the relationship between the partial pressure of a gas above a liquid solution and the concentration of that gas dissolved in the liquid at a constant temperature.
• Mathematically, Henry's law is expressed as 𝑃=𝑘𝐻⋅𝑥P=kH​⋅x, where:
  • 𝑃P is the partial pressure of the gas above the solution,
  • 𝑘𝐻kH​ is Henry's constant, which is specific to the gas-solvent system and depends on temperature,
  • 𝑥x is the mole fraction of the gas in the liquid phase.
• In simpler terms, Henry's law states that the partial pressure of a gas above a solution is directly proportional to the concentration (mole fraction) of that gas dissolved in the liquid phase.
• This means that as the concentration of the gas in the liquid phase increases, the partial pressure of the gas above the solution also increases proportionally.
• Henry's law is particularly relevant in gas-liquid equilibria, such as in processes like gas absorption and stripping, where the concentration of a gas in a liquid phase is important for understanding mass transfer phenomena.