Regarding to Henry's law which of the following is not correct statement ?

Question

Regarding to Henry's law which of the following is not correct statement ? (A) Different gases have different KH (Henry's law constant) values at the same temperature (B) The partial pressure of the gas in vapour phase is proportional to the mole fraction of the gas in the solution (C) Higher the value of KH at a given pressure, higher is the solubility of the gas in the liquids (D) The value of KH increases with increase of temperature and KH is function of the nature of the gas

Tardigrade Admin · Accepted Answer

p=KH× x Where KH= Henry law constant Henry's constant increases with increase in temperature while it decreases with increase in solubility. Hence, value of KH increases as solubility of gas increases is a wrong statement.

Q. Regarding to Henry's law which of the following is not correct statement ?

Different gases have different $K_{H}$ (Henry's law constant) values at the same temperature

The partial pressure of the gas in vapour phase is proportional to the mole fraction of the gas in the solution

Higher the value of $K_{H}$ at a given pressure, higher is the solubility of the gas in the liquids

The value of $K_{H}$ increases with increase of temperature and $K_{H}$ is function of the nature of the gas

$p = K_{H} \times x$
Where $K_{H} =$ Henry law constant
Henry's constant increases with increase in temperature while it decreases with increase in solubility. Hence, value of $K_{H}$
increases as solubility of gas increases is a wrong statement.

Q. Regarding to Henry's law which of the following is not correct statement ?

Different gases have different KH​ (Henry's law constant) values at the same temperature

The partial pressure of the gas in vapour phase is proportional to the mole fraction of the gas in the solution

Higher the value of KH​ at a given pressure, higher is the solubility of the gas in the liquids

The value of KH​ increases with increase of temperature and KH​ is function of the nature of the gas

p=KH​×x Where KH​= Henry law constant Henry's constant increases with increase in temperature while it decreases with increase in solubility. Hence, value of KH​ increases as solubility of gas increases is a wrong statement.

Different gases have different $K_{H}$ (Henry's law constant) values at the same temperature

Higher the value of $K_{H}$ at a given pressure, higher is the solubility of the gas in the liquids

The value of $K_{H}$ increases with increase of temperature and $K_{H}$ is function of the nature of the gas

$p = K_{H} \times x$
Where $K_{H} =$ Henry law constant
Henry's constant increases with increase in temperature while it decreases with increase in solubility. Hence, value of $K_{H}$
increases as solubility of gas increases is a wrong statement.