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Which one of the following statements regarding Henry's law is not correct? (1) Different gases have different K_H (Henry's law constant) values at the same temperature. (2) The partial pressure of the gas in vapour phase is proportional to the mole fraction of the gas in the solution. (3) The value of K_H increases with increase of temperature and K_H is a function of the nature of the gas. (4) Higher the value of K_H at a given pressure, higher is the solubility of the gas in the liquids.

1. Different gases have different K_H (Henry's law constant) values at the same temperature.
2. The partial pressure of the gas in vapour phase is proportional to the mole fraction of the gas in the solution.
3. The value of K_H increases with increase of temperature and K_H is a function of the nature of the gas.
4. Higher the value of K_H at a given pressure, higher is the solubility of the gas in the liquids.

Correct answer: Higher the value of K_H at a given pressure, higher is the solubility of the gas in the liquids.

Solution

By Henry's law p = K_H * x, so x = p/K_H. At a given pressure a larger K_H gives a smaller mole fraction, i.e. lower solubility. Hence the statement that higher K_H means higher solubility is the incorrect one.

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