Henry's Law is an important concept in the study of solutions and gases, especially in chemistry for Class 12. It describes the relationship between the pressure of a gas above a liquid and the concentration of the gas dissolved in the liquid. The law states:
Henry's Law:
"The solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the surface of the liquid, provided the temperature remains constant."
Mathematically, Henry’s Law is expressed as:
\[C = k_H \cdot P\]
Where:
- \(C\) = Concentration of the gas in the solution (solubility)
- \(P\) = Partial pressure of the gas
- \(k_H\) = Henry’s Law constant (which depends on the nature of the gas and the solvent, and the temperature)
Key Points:
1.Effect of Pressure As the pressure of a gas above a liquid increases, the solubility of the gas in the liquid also increases.
2. Effect of Temperature Generally, the solubility of gases decreases with an increase in temperature.
3. Applications
- Scuba diving: At higher pressures under water, more nitrogen dissolves in the bloodstream, which can lead to conditions like nitrogen narcosis or "the bends" (decompression sickness) when resurfacing.
- Carbonated drinks: CO₂ is dissolved in drinks under high pressure, and when the bottle is opened, the pressure decreases, causing the gas to come out of solution, leading to fizzing.
Limitations of Henry’s Law:
- It is valid only for gases that do not react chemically with the solvent.
- It works well for gases at low concentr
.jpeg)
0 Comments