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Henry's Law Equation:
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Henry's Law states that the amount of dissolved gas in a liquid is proportional to its partial pressure above the liquid. For CO2 in water, this relationship is expressed as P_CO2 = K_H × C_CO2, where P_CO2 is the partial pressure, K_H is Henry's constant, and C_CO2 is the concentration of dissolved CO2.
The calculator uses Henry's Law equation:
Where:
Explanation: The equation demonstrates the linear relationship between the partial pressure of a gas above a solution and its concentration in the solution.
Details: Calculating partial pressure of CO2 in water is crucial for understanding carbonation processes, aquatic ecosystems, blood gas exchange, and various industrial applications including beverage production and environmental monitoring.
Tips: Enter Henry's constant in Pa·m³/mol and CO2 concentration in mol/m³. Both values must be positive numbers. Note that Henry's constant varies with temperature.
Q1: What is the typical value of Henry's constant for CO2?
A: At 25°C, Henry's constant for CO2 is approximately 29.4 Pa·m³/mol, but it varies with temperature.
Q2: How does temperature affect Henry's constant?
A: Henry's constant generally increases with temperature, meaning less gas dissolves at higher temperatures at the same partial pressure.
Q3: Can this calculator be used for other gases?
A: Yes, the same principle applies to other gases, but you need to use the appropriate Henry's constant for each specific gas.
Q4: Why is partial pressure important in aquatic environments?
A: Partial pressure of CO2 affects pH levels, carbonate equilibrium, and overall chemical balance in aquatic systems, impacting marine life and ecosystem health.
Q5: How is this relevant to human physiology?
A: Henry's Law governs gas exchange in lungs and tissues, making it fundamental to understanding respiratory physiology and blood gas transport.