1. What is Henry's Law Constant?

Definition: Henry's Law Constant (K_H) is a measure of the concentration of a chemical in air over its concentration in water at equilibrium.

Purpose: It helps quantify how much of a gas will dissolve in a liquid at a given pressure, important in environmental chemistry and chemical engineering.

2. How Does the Calculator Work?

The calculator uses the formula:

Where:

• \( K_H \) — Henry's Law Constant (Pa·m³/mol)
• \( P_{partial} \) — Partial pressure of the gas (Pascal)
• \( x_{liquid} \) — Mole fraction of the component in liquid phase (dimensionless)

Explanation: The constant is calculated by dividing the partial pressure of the gas above the solution by the mole fraction of the gas dissolved in the liquid.

3. Importance of Henry's Law Constant

Details: This constant is crucial for understanding gas solubility in liquids, designing aeration systems, and studying environmental processes like gas exchange between atmosphere and water bodies.

4. Using the Calculator

Tips: Enter the partial pressure in Pascals and mole fraction (between 0 and 1). The mole fraction represents the ratio of moles of dissolved gas to total moles in solution.

5. Frequently Asked Questions (FAQ)

Q1: What are typical units for Henry's Law Constant?
A: Common units are Pa·m³/mol, atm·m³/mol, or dimensionless depending on the form of Henry's Law used.

Q2: How does temperature affect Henry's Constant?
A: K_H increases with temperature - gases become less soluble in liquids at higher temperatures.

Q3: What's a typical value for common gases?
A: For CO₂ at 25°C it's about 0.034 mol/L·atm, while for O₂ it's about 0.0013 mol/L·atm.

Q4: Can this be used for any gas-liquid system?
A: It works best for dilute solutions where the gas doesn't react with the solvent.

Q5: How is this different from solubility?
A: While related, solubility is typically expressed as concentration, while Henry's constant relates partial pressure to mole fraction.