I don’t understand the pressure during the chlorine drying process
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I am revising my graduation project and there are two points I don’t understand; I hope everyone can offer some guidance. For wet chlorine gas as it passes from the electrolyzer to a titanium cooler, there is a problem of calculating the amount of dissolved chlorine gas using Dalton’s law of partial pressures. The original text states that \"since the total pressure in the system is -98.07 Pa, it can be considered as 101.227 kPa for calculations. According to Dalton’s law of partial pressures: P_water/P_total = n_water/n_total.\" Why can 1 standard atmosphere be used in place of this value here? Another question is: “(2) In a titanium cooler, the temperature of chlorine drops from 80°C to 46°C. Suppose the amount of water that condenses in the first titanium cooler is W2 kg, and the pressure drop is 35×9.81 Pa; then the total pressure of the chlorine at the outlet is -40×9.81 Pa. Therefore, P_total = 101.227 – 35×9.81×10^-3 = 100.933 kPa.” How is this outlet pressure of chlorine calculated?
I am working on the design of a roller kiln for daily-use porcelain, and I’m looking for some sample diagrams as reference. Email: 2730855438@qq.com
What does the original text refer to? Where did you see it? Where does the original text come from? What does that document say?
The original text is a graduation thesis titled \"Preliminary Design for an Annual Production Capacity of 200,000 Tons of Caustic Soda, Chlorine, and Hydrogen.\" It relates to the calculation of chlorine; specifically, it deals with the calculation of chlorine from the electrolyzer to the first titanium cooler. This can be found on page 9 at http://www.docin.com/p-1656235415.html