Henryvergelijking
The Henryvergelijking, also known as Henry's Law, is a fundamental principle in physical chemistry that describes the relationship between the concentration of a gas in a liquid and its partial pressure above the liquid. It is named after the English chemist William Henry, who formulated the law in 1803. The law states that the amount of a gas dissolved in a liquid is directly proportional to the partial pressure of that gas above the liquid, provided the temperature remains constant.
Mathematically, Henry's Law can be expressed as:
- C is the concentration of the gas in the liquid (in moles per liter or mol/L),
- P is the partial pressure of the gas above the liquid (in atmospheres or atm),
- k is the Henry's Law constant, which is specific to the gas and the liquid at a
The Henry's Law constant, k, varies with temperature and is often determined experimentally. It is typically
Henry's Law has several important implications:
1. It explains why gases dissolve more readily in liquids at higher pressures.
2. It helps in predicting the behavior of gases in aquatic environments, such as the solubility of
3. It is used in the design of gas absorption and desorption processes in industrial applications.
Despite its simplicity, Henry's Law provides a valuable framework for understanding the interaction between gases and