State and explain Henry’s law.

Henry's law states that at a constant temperature, the amount of gas that dissolves in a liquid is directly proportional to the partial pressure of that gas above the liquid. This means that if the pressure of the gas increases, more gas will dissolve into the liquid, and if the pressure decreases, less gas will dissolve. This principle is essential in understanding gas solubility in liquids, such as carbonated beverages, where carbon dioxide is dissolved in the liquid under high pressure.

Henry's law is a fundamental principle in chemistry that describes how gases behave when they are in contact with liquids. Specifically, it states that the quantity of a gas that can dissolve in a liquid at a constant temperature is directly related to the pressure of that gas above the liquid.

Key Concepts of Henry's Law

• Direct Proportionality: As the partial pressure of the gas increases, the amount of gas that dissolves in the liquid also increases.
• Temperature Dependency: This relationship holds true only at a constant temperature; changes in temperature can affect solubility.
• Practical Applications: This law is crucial for understanding phenomena like the carbonation in soft drinks, where carbon dioxide is dissolved under high pressure.

Real-World Example

In carbonated beverages, carbon dioxide gas is infused into the liquid under high pressure. When you open the bottle, the pressure decreases, leading to the release of gas bubbles as the dissolved carbon dioxide escapes. This illustrates Henry's law in action, showing how pressure influences gas solubility.