Question

According to Henry's law, the partial pressure of gas $\left(P_g\right)$ is directly proportional to mole fraction of gas in liquid solution, $P_{gas}=K_H.X_{gas}$, where $K_H$ is Henry's constant. Which is incorrect?

• A. $K_H$ is characteristic constant for a given gas-solvent system at given temperature
• B. Higher is the value of $K_H$, lower is solubility of gas for a given partial pressure of gas
• C. $K_H$ has temperature dependence
• D. $K_H$ decreases with increase of temperature

Answer 1

Answer: (C)

$K_H$ has temperature dependence

$P_{gas}=K_H.X_{gas}{K}_H\to Henr{y}^{\prime }s$ Constant and independent of temperature

It is the measurement of solubility. More it is more is the solubility.

But it does not depend upon temperature. On increase and decrease of

temperature partial pressure of gas of $X_{gas}$ varies only keeping $K_H$ constant.