Solubility of a Gas and Temperature Relationship

Introduction:
Solubility of a gas in a liquid is the maximum amount of gas that can be dissolved in the liquid at a particular temperature and pressure. The solubility of gases in liquids depends on several factors, such as temperature, pressure, and the nature of the gas and the liquid. One of the most important factors affecting the solubility of gases in liquids is temperature. This article will explain whether the statement "Solubility of a gas increases with increase in temperature" is true or false.

Explanation:
The statement "Solubility of a gas increases with increase in temperature" is false. The solubility of gases in liquids is generally inversely proportional to temperature. In other words, when the temperature of a liquid increases, the solubility of gases in it decreases. This relationship is known as the Henry's law.

The Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. In other words, the higher the pressure of the gas, the more gas molecules will be dissolved in the liquid. However, this relationship is only true at a constant temperature. If the temperature of the liquid changes, the solubility of the gas will also change.

When the temperature of a liquid increases, the kinetic energy of the gas molecules also increases. This leads to an increase in the average speed of the gas molecules, which reduces the chances of them being dissolved in the liquid. As a result, the solubility of gases in liquids decreases with increasing temperature.

Conclusion:
In conclusion, the statement "Solubility of a gas increases with increase in temperature" is false. The solubility of gases in liquids generally decreases with increasing temperature. This relationship is known as the Henry's law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid at a constant temperature.