For the solubility of gases in liquid, the correct statement at high temperature is:

A. Solubility of gases increase

B. Value of Henry's constant \((K_H)\) increases

C. Solubility of gases decreases

D. Value of \(K_H\) decreases

E. Value of \(K_H\) does not change

Choose the correct answer from the options given below:

B and C only

The correct answer is option 4. B and C only.

At high temperatures, the solubility of gases in liquids generally decreases. This is because when you increase the temperature:

1. Kinetic energy increases: The molecules in both the gas phase and the liquid phase gain more kinetic energy. Gas molecules move more rapidly, and liquid molecules also move faster, disrupting the intermolecular forces that keep the gas molecules dissolved.

2. Increased molecular motion disrupts solvation: The increased kinetic energy disrupts the intermolecular forces between gas molecules and solvent molecules. This disruption weakens the solvation process, making it easier for gas molecules to escape from the liquid phase into the gas phase.

Regarding Henry's Law constant (\(K_H\)):

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 that gas above the liquid. Mathematically, this relationship is represented by:

\(C = K_H \times P \)

where:

\(C\) is the concentration of the gas in the liquid (solubility),

\(K_H\) is Henry's Law constant,

\(P\) is the partial pressure of the gas.

At higher temperatures, as the solubility of gases decreases, the value of Henry's constant (\(K_H\)) also decreases. This is because the equilibrium between the gas phase and the dissolved gas in the liquid phase shifts towards the gas phase due to decreased solubility.

So, at high temperatures, the correct statements are:

C. Solubility of gases decreases.

D. Value of Henry's constant (\(K_H\)) decreases.