Problem 126 Which of the following would inc... [FREE SOLUTION] (2024)

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Henry's Law is a critical principle in understanding gas solubility, especially in liquid solutions. This law states that at a constant temperature, the amount of gas that can be dissolved in a liquid is directly proportional to the partial pressure of the gas above the liquid.
Essentially, if the pressure of a gas above a liquid increases, more gas molecules are ‘pushed’ into the solution.
The mathematical representation of Henry's Law is: \( C = kP \)
where:

\( C \): concentration of the gas in the liquid
\( k \): Henry's Law constant
\( P \): partial pressure of the gas above the liquid

This relationship helps predict how changes in pressure will affect the solubility of a given gas.

Gas solubility refers to how much of a gas can dissolve in a liquid at a given temperature and pressure.
Different gases have different solubility levels in liquids. Factors like temperature, pressure, and the nature of the gas and liquid can affect solubility.
Here are some key points to note:

• Simpler gases tend to be more soluble than more complex ones.
• The solubility of gases decreases with the increasing complexity of the gas molecules.
• Gases are generally less soluble in organic solvents than in water.

Understanding gas solubility is fundamental for various scientific fields, including chemistry, environmental science, and engineering.

Pressure plays a significant role in determining the solubility of gases in liquids. According to Henry's Law, increasing the pressure of a gas above a liquid increases its solubility in that liquid.
Here's how:

• When pressure increases, gas molecules are forced into the liquid.
• This results in a higher concentration of the gas in the solution.

Conversely, decreasing the pressure results in lower solubility because fewer gas molecules are pushed into the liquid.
For example, in carbonated drinks, carbon dioxide is dissolved in the beverage under high pressure. When you open the bottle, the pressure decreases, and the gas starts to escape, forming bubbles.

Temperature is another crucial factor that affects the solubility of gases in liquids. Generally, increasing the temperature decreases gas solubility.
Here's why:

• Higher temperatures give gas molecules more kinetic energy.
• This energy allows them to escape from the liquid more easily.

On the other hand, lower temperatures reduce the kinetic energy of gas molecules, making them less likely to escape and more likely to remain dissolved.
This principle is important in various practical applications. For example, in aquatic environments, warmer water holds less dissolved oxygen compared to cooler water, which can affect marine life.
Understanding this concept helps in fields like environmental science and chemical engineering.