Temperature affects both the equilibrium position of the precipitation reaction and the reaction rate. In general, solubility increases with the increasing temperature with a few notable exceptions such as CaCO3, Ca3(PO4)2, CaSO4 and FePO4 which are of importance in the water chemistry. To calculate the solubility at a temperature with the equation in the picture
We discussed that the CO2 absorption into water would depend largely on its solubility and hence involved the principles of mass transfer. Hence, we sought advice from Dr Lee on the transfer of CO2 into water. His advice led us to finding the book: Perry’s Chemical Engineer’s Handbook 8th Edition- Don W. Green & Robert H. Perry.
According to research P = H.x
Where P is the partial pressure of the solute in the gas phase
H is the henry’s constant
And x is the mole fraction of the solute in the liquid phase.
We are having several questions and confusion about these since we do not know the total pressure of the biogas introduced and we assume that the temperature is at room temperature. We are also unable to find the mole fraction of the solute in the liquid phase which hence does not allow us to determine the partial pressure of the solute in the gas phase. Other factors for example, ionic equilibrium, has also jumped across out minds due to the reaction of CO2 and water.
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