Henry's Law Formula:
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Definition: Henry's Law Constant is the ratio of a compound's partial pressure in vapor phase to the concentration of the compound in liquid phase at a given temperature.
Purpose: It helps quantify the solubility of gases in liquids and is widely used in environmental chemistry, chemical engineering, and atmospheric sciences.
The calculator uses the formula:
Where:
Explanation: The partial pressure of the gas is divided by its concentration in the liquid phase to determine the Henry's Law constant.
Details: This constant is crucial for understanding gas solubility, designing gas-liquid separation processes, and modeling environmental fate of volatile compounds.
Tips: Enter the partial pressure in Pascals and concentration in mol/m³. Both values must be > 0.
Q1: What are typical units for Henry's Law constant?
A: Common units are mol/m³·Pa, though atm·m³/mol is also used (different form of the law).
Q2: How does temperature affect Henry's constant?
A: Generally, the constant increases with temperature as gas solubility decreases.
Q3: What's a typical value for common gases?
A: For CO₂ at 25°C it's about 3.3×10⁻⁴ mol/m³·Pa, while for O₂ it's about 1.3×10⁻⁵ mol/m³·Pa.
Q4: When would I need to calculate this constant?
A: When designing aeration systems, studying gas exchange in water bodies, or modeling chemical processes.
Q5: 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.