Question

According to Henry’s Law, in gases, an increase in pressure increases:

• A. Solubility
• B. Saturation
• C. Volume
• D. Viscosity

Hint:

When pressure increases, the gas molecules are forced into the solution, leading to higher solubility.

Answer 1

The Correct Option is A

Step 1: Concept.
Henry's law is written as p = KH x, where x is the mole fraction of dissolved gas and KH is constant at a fixed temperature.

Step 2: Apply it.
Since x = p / KH, a rise in pressure p directly raises x, and x is exactly what we mean by the gas's solubility in the liquid.

Step 3: Final Answer.
Increasing pressure increases the Solubility of the gas.

Answer 2

A familiar example makes this easier to check than the equation alone, a sealed bottle of a carbonated drink.

1. Solubility: A soft drink bottle is sealed under high carbon dioxide pressure, which is exactly why it can hold so much dissolved gas. Once opened, the pressure drops and the gas comes bubbling out because less of it can stay dissolved at lower pressure. This shows solubility rising and falling with pressure, in line with Henry's law.
2. Saturation: Opening the bottle does change how full the drink is with gas, but that is a consequence of the change in dissolved amount, not something Henry's law names directly as the quantity that scales with pressure.
3. Volume: The liquid volume in the bottle does not change when it is opened, so pressure is clearly not acting on liquid volume here.
4. Viscosity: The drink does not become thicker or thinner when the cap is removed, so viscosity is not the property being affected.

The fizzing on opening a bottle is dissolved gas leaving because solubility fell when pressure fell, exactly as Henry's law states.

So the correct answer is Solubility.