Question

state henrys law why do gases nearly always tennd to be less soluble liquids as the tempreture is mised

Answer 1

Henry's Law indicates that gas solubility in liquids is directly proportional to pressure; however, gas solubility decreases as temperature increases due to higher kinetic energy encouraging the gas to escape from the liquid.

Step-by-step explanation:

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. As temperature increases, the kinetic energy of the gaseous solute also increases, which encourages the gas molecules to escape from the solvent into the gas phase, leading to a decrease in gas solubility. In contrast to solids and liquids, whose solubility typically increases with temperature, gases nearly always tend to be less soluble in liquids as the temperature rises.

This behavior is confirmed by observing substances such as HCl, NH3, and SO2. These gases have decreased solubility in liquid solvents at elevated temperatures because their increased kinetic energy overcomes the intermolecular forces that previously kept them dissolved. The effect of temperature on gas solubility is analogous to the increase in vapor pressure with temperature, where added thermal energy overcomes attractive forces between solvent molecules in the case of vapor pressure.

Thus, understanding the relationship between temperature, pressure, and solubility is key to many processes, including industrial applications where gases are dissolved in liquids, and environmental considerations where temperature changes can influence the solubility of gases in natural waters.

Answer 2

Henry's Law explains that the solubility of gases in liquids decreases with rising temperatures due to increased kinetic energy that encourages gas molecules to escape into the gas phase. Heating a solution can overcome intermolecular attractions, resulting in lower solubility.

Step-by-step explanation:

Henry's Law and Solubility of Gases

According to Henry's Law, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. This principle can be observed in substances like HCl, NH3, and SO2, which are gases at standard temperature and pressure and display reduced solubility as temperature increases. As temperature rises, the kinetic energy of solute and solvent molecules increases, leading to a higher likelihood of gas molecules escaping from the solvent and returning to the gas phase. Therefore, increased temperature generally results in decreased gas solubility in liquids. This behavior contrasts with that of most solid or liquid solutes, whose solubility typically increases with temperature.

Additionally, it is important to note that intermolecular forces play a significant role in the solubility of gases. When a gas dissolves in a liquid, it is due to the interaction between gas molecules and solvent molecules. Dissolving gases is typically an exothermic process, and applying heat to the solution can provide enough energy to overcome these attractive forces, decreasing gas solubility. Understanding the phase behavior in relation to temperature, we observe that substances transition from solid to liquid to gas as the temperature increases.