Henry's Law

Question

Henry's Law constant (kH) for O2 increases with temperature. Solubility of O2 in water will:

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1. **Henry's Law Equation**: $P = K_H 	imes X$, where $P$ is the partial pressure of the gas and $X$ is the mole fraction (solubility) of the gas in the liquid.
2. **Relative Relationship**: At a constant pressure ($P$), the solubility $X$ is inversely proportional to the Henry's Law constant ($X = \frac{P}{K_H}$).
3. **Temperature Effect**: As **Temperature increases**, the kinetic energy of gas molecules increases, helping them escape the liquid phase. This is reflected in an **increase in $K_H$**.
4. **Conclusion**: Since $K_H$ increases with temperature, the solubility ($X$) must **decrease**. This explains why aquatic life is more comfortable in cold water (higher dissolved $O_2$) than in warm water.

Henry's Law

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