Given below are two statements:
Statement-I: \( K_H \) is constant with change in concentration of gas till solution is dilute at a given temperature.
Statement-II: According to Henry’s Law, partial pressure of gas in vapor phase is inversely proportional to mole fraction of gas in solution.
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Remember that Henry's law describes the solubility of a gas in a liquid, where the solubility is directly proportional to the partial pressure of the gas.
Statement-I is incorrect and Statement-II is correct
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The Correct Option isC
Solution and Explanation
Let's analyze each statement individually to determine their correctness in the context of Henry's Law:
Statement-I: \( K_H \) is constant with change in concentration of gas till solution is dilute at a given temperature.
Henry's Law states that at a constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas over the liquid. This relationship is mathematically expressed as \( P = K_H \times x \), where \( P \) is the partial pressure, \( K_H \) is Henry's Law constant, and \( x \) is the mole fraction of the gas.
The constant \( K_H \) is specific for a particular gas-solvent pair and remains constant as long as the temperature is constant and the solution is diluted. Thus, Statement-I is correct.
Statement-II: According to Henry’s Law, the partial pressure of gas in vapor phase is inversely proportional to mole fraction of gas in solution.
As mentioned, Henry's Law indicates a direct proportionality between the partial pressure of a gas and its mole fraction in a solution: \( P = K_H \times x \).
Since this relationship is direct, not inverse, Statement-II is incorrect because it incorrectly states an inverse relationship.
Based on the above analysis, the correct choice is: Statement-I is correct, Statement-II is incorrect.
