Talk:Oxygen solubility: Difference between revisions

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== Calculations ==
::::* [[File:O2 concentratio and pressure in closed system with change of temperature.xlsx]]
== Fundamentals in short ==
== Fundamentals in short ==



Latest revision as of 10:14, 26 October 2022

Calculations

Fundamentals in short

The ideal gas law plays a central role in elucidating the behavior of gases dissolved in aqueous solution, where O2 interacts with a very different environment compared to the gas phase.
Eq. 1:  cG(g) = pGยท(RT)-1 
The gas law (Eq. 1) is called 'ideal', since the activity coefficient ฮณG(g) of an ideal gas G is defined as zero. Actually, the molar volume Vm,G(g) = 1/cG of the ideal gas is 22.414 L/mol at 0 ยฐC, whereas the real molar volume of O2 is Vm,O2(g) = 22.392 L/mol at 0 ยฐC. The ratio Vm,G(g)/Vm,O2(g) is ฮณO2(g) = 22.414/22.392 = 1.001. Therefore, O2(g) behaves closely as an ideal gas at practically encountered barometric pressures. In aqueous solution, O2(aq) has a much higher activity coefficient ฮณO2(g). Defining solubility as concentration per pressure, rearranging Eq. 1, and inserting the activity coefficient ฮณO2(aq) yields,
Eq. 2a:  SG(g) = cG(g)ยทpG-1 = (RT)-1


Eq. 2b:  ฮณO2(aq)ยทSO2(aq) = ฮณO2(aq)ยทcO2(aq)ยทpO2-1 = (RT)-1 
The partial pressures of a gas in the gas phase and aqueous phase are equal at equilibium between the two phases. Pressure is general at practically encountered pressures (fugacity is the more general concept applicable in the deep sea), such that the partial pressure of an ideal gas pG can be set equal to the partial pressure of a real gas pO2. Therefore, ฮณO2(aq) is derived as
Eq. 3:  ฮณO2(aq) = cG(g)/cO2(aq) = SG(g)/SO2(aq) 


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