Question

State Henry’s Law regarding the solubility of gases in liquids and mention two daily-life applications.

Hint:

Higher pressure increases gas solubility, while higher temperature usually decreases it.

Answer 1

Concept: Henry’s Law explains how gases dissolve in liquids under pressure. It is important in chemistry, environmental science, and many real-life situations involving gas-liquid equilibrium.
Statement of Henry’s Law: At constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
Mathematical Expression: \[ p \propto x \] or \[ p = k_H x \] where,
\( p \) = partial pressure of the gas
\( x \) = mole fraction (solubility) of gas in liquid
\( k_H \) = Henry’s Law constant

Daily-Life Applications:
Carbonated Beverages: Soft drinks are bottled under high pressure so that more \( CO_2 \) dissolves in the liquid. When opened, pressure decreases and gas escapes as fizz.
Deep-Sea Diving: Divers use special gas mixtures because high pressure increases nitrogen solubility in blood. Rapid ascent can cause nitrogen bubbles (decompression sickness).