Chlorine & Hydrogen Psychrometric or Mollier Chart

other alternatives, hire a chemical engineer.

Why?

U better post this question in "Chemical & Material Science" section

In Oil & Gas/Petrochemical/Chemical industry... We mechanical engineers follow your (chemical engineer) advise. We don't advise or question chemical engineers :-D

Cheers

You can work it out from the water vapour at the temperature. Mass of vapour per m3 doesn't depend on the type of gas or total pressure. Same figure if it's a vacuum.

You may want to consider that what you are looking for is an oxymoron. It was Dalton, a Manchester schoolteacher in 1802, who announced his conclusion that the vapor pressure of water in air is independent of the existence of air The same results are obtained in a vacuum.

Well I searched the word 'psychrometric' & it was more frequent in Mechanical as compared to Chemical section

OK, but have you now got the information you need?

I certainly hope you can keep these two gases apart and away from UV/visible light, to avoid the instant detonation. Chlorine you cannot dry out completely, and you will have to use advanced techniques, some of the moisture will come out at sufficiently low temperature with chlorine dissolved in it (extremely corrosive), and at about the same temperature chlorine may turn into a liquid if the pressure is sufficient. I don't think the pressure is any where near the liquidus in your case.

Hire a chemical engineer with experience in the chlor-alkali process, that is your best option. Otherwise, you are simply planning for a big mistake.

I wouldn't expect the gases to be mixed, as they are released at different points of the electrolytic cell. OP referred to 2 coolers.

We could probably help him more if he wanted, but he hasn't been back.

Yes sir you got that right we have separate coolers one for Cl2 (that comes from anode compartment) & one for H2 (that comes from cathode). In either case lot of brine & caustic (because electrolysis is occuring at ~88celsius) is entrained in Cl2 & H2 respectively this can be acknowledged by the condensate collected amount in buffer tanks of both H2 & Cl2.

The idea is simple:

Assuming that Cl2 leaves cell compartment at nearly same temperature (88) at that temperature what is the maximum amount of moisture it can hold up, before it gets saturated & brine entrained will no longer travel with it. The gas headers (ID 200mm) are slightly inclined for condensate to travel back to cell compartments.

Nightcrawler

Did this tell you what you wanted? Or better, did the water flow in practice turn out as calculated? How did you get on with the hydrogen calculation?

Thanks I will post my calculations within two days however

So if mass flow of Cl₂ = q kg/s, total volume flow = q/1.29 m³/s

this q refers to total flow Cl2 + vapours & not just Cl2? I must also mention that at a given current load say 40kAmp I can easily calculate H2/Cl2 production using Faraday law but in our process stream there is no totaliser in Cl2 pipeline telling us total flow of Cl2 + vapours

And yes we have demisters installed in Cl2 pipeline

That's correct, total flow before cooling = q/1.29.

I should have said in #11 - the total volume flow after the cooler is roughly half the total flow before (though after the cooler it's nearly all chlorine if cooled to something like 10°C).

You do know something about the rate of product accumulation, do you not? Also, you could measure hydrogen flow (mass flow and volumetric flow) since that is non-corrosive, and use the stoichiometric relationship to determine precise data for chlorine. How do you actually arrive at completely dry chlorine liquid in the bottle?

You brits! Your mole is precisely 1000 times the mole I learned in high school! Threw me for a loop, didn't you?

Over here in the states, 1 mole of gas at 760mmHg and 273.15 °K (0 °C, for those in Rio Linda) is 22.4 L (molar volume). But you also stated 1000 millibar, which is 750.1 mm Hg, thus the molar volume at that pressure is 22.7 L (for 71 g chlorine, or for 18 g water), but you are using Kgmol unit, thus since 1 L = 0.001 m³, the stated Molar Volume v is correct at 22.7 m³ represents 71 Kg chlorine, or 18 Kg water.

Being somewhat dim-witted this morning, I also had a temporary problem understanding your volume flow, and water mass flow calculation, but it's all good.

I prefer to use molar volume at 1 bar rather than 1 atm, as I usually have pressure in bar. That's 22.7m³ at 0°C, something different again at 15 or 20°C or maybe 68°F that you guys over there go for! As you say, 22.4m³ at 1 atm and 0°C, as I also remember from school (long distant).

For moles, molecular weights are really just ratios (originally to the mass of an hydrogen atom, then to 1/16 mass of an O2 atom, now to 1/12 mass of a carbon atom (as I'm sure you know). I prefer to think of it that way, so eg water = 18. When I see 0.018 kg/mole I have to stop and think and it interrupts my train of thought. Of course it's the same as 18 kg/kmole. But I usually do a check to ensure I'm not out by 1000.

It is still nice to be able to converse well across the pond (and back).