Question

Which is correct about Henry’s law?
A) The pressure should not be too high
B) The temperature should not be too low
C) The gas should not dissociate neither enter into chemical combination with solvent
D) All of these

Answer 1

Hint:Henry law states that the amount of gas that has been dissolved in a liquid is directly proportional to the partial pressure of the gas above the liquid when the temperature is constant.


Complete step by step solution:
The formula used in Henry’s law is
$P={{k}_{H}}.C$
Where, $P$ is the partial pressure of the gas above the liquid
$C$ is the concentration of the gas
${{k}_{H}}$ denotes Henry’s law constant
Let us discuss the option given that is valid for Henry law:
1) Henry law is not applicable for gases that work under very high pressure. If the pressure is increased, the pressure of atmospheric gases also increases, that is nitrogen gas is increased, the solubility also increases and becomes harmful when in the blood supply. Therefore option A. Is correct
2) Henry law is applicable only when a gas behaves like an ideal gas. Ideal gases are the gases that have no attraction between the gas molecule. When the pressure is high and molecules are close to each other, attraction takes place between the gas molecules. To remove this attraction temperature is increased so that molecules move with greater speed. Therefore option B. Is also correct.
3) Henry law is not applicable when gases react chemically with solvent or dissociate with solvent. Therefore option C. Is also correct.

Therefore option D. is the correct option that is all of these.


Note:In this question we have discussed Henry law that states that the concentration of the gas is directly proportional to the partial pressure of the gas.It is a thermodynamic law that gives an explanation of dissolution of gas in a liquid medium.