Question

Under which of the following conditions, the gases does not follow Henry's law?

• A. When gases are placed under high temperature.
• B. When the molecules of the system are in equilibrium state.
• C. When gases are placed under extremely high pressure.
• D. All of the above

Hint:

Henry's law is applicable at low pressures and temperatures. At high pressures or temperatures, gases may not follow Henry’s law due to deviations from ideal behavior.

Answer 1

The Correct Option is C

Henry's Law states that the amount of gas dissolved in a liquid is directly proportional to the partial pressure of the gas above the liquid, at a constant temperature. Mathematically, it is expressed as: \[ C = k_H P \] Where:
- \( C \) is the concentration of the gas in the solution,
- \( k_H \) is the Henry’s law constant,
- \( P \) is the partial pressure of the gas. However, Henry's law holds true under certain conditions: 1. High temperatures can cause deviations from Henry’s law because the solubility of gases typically decreases with increasing temperature.
2. Equilibrium state refers to the situation where the gas and the solution are in equilibrium, and Henry’s law applies here.
3. Extremely high pressures lead to deviations because the gas molecules behave non-ideally at very high pressures, causing the gas to deviate from Henry’s law. At such high pressures, the interactions between gas molecules become significant, leading to deviations from the ideal behavior assumed by Henry's law. Therefore, the correct answer is option (c).