Can some one give me the evaporation rate of hydrochloric acid a
R & D Team - C User
I am a chemical engineer and working at Tata Chemicals Limited, Gujarat,
India. Our company is the largest manufacturer of Synthetic Soda Ash in
Asia.
I require following information.
What is the evaporation rate of hydrochloric acid at 40 degree celcius and
atmospheric pressure?
I require this information to design the scrubber for HCL fumes.
Regards,
Anish K Shah
Uncle Al
It depends on the concentration of HCl and mass transfer (wind) at the
interface, assuming an infinite thermal source. One expects there to
be a relative humidity term in there, too. Vapor pressure of constant
boiling (12 M) HCl vs. temp should be well tabulated in the
literature, probably other concentrations as well.
It's one of those things were you can simulate until you are blue in
the face, and will wind up making real world measurements and
optimizations anyway. Start with vapor pressure data and go right to
bench scale testing. You will get real world data at minimum overall
cost. Scrubber design should be in both the professional and the
patent literature, including the mist problem.
Worry about corrosion. Worry about corrosion a lot! Halide is the
universal corrosive agent. HCl + air eats even gold.
--
Uncle Al
http://www.mazepath.com/uncleal/eotvos.htm
(Do something naughty to physics)
Gerard Westendorp
> What is the evaporation rate of hydrochloric acid at 40 degree Celsius and
> atmospheric pressure?
>
> I require this information to design the scrubber for HCL fumes.
Thermodynamics can give you the vapor pressure above the liquid. If it
is bigger that 1 atmosphere, the liquid will be boiling, so the
evaporation rat is infinite, provided you can maintain the specified
temperature. In practice of course, the temperature will drop to
the boiling point or very slightly lower, and the evaporation rate
is limited by the heating rate.
If the vapor pressure is below 1 atmosphere, the evaporation rate
can in principle be zero, if you have a layer of saturated vapor
above the fluid. There is equilibrium and nothing happens on a
macroscopic scale.
In practice you often have the vapor being flushed away for example
by air. The evaporation rate then depends on how the air flushes the
liquid surface. There is a lot of literature on this: look up a
chapter on evaporators in a chemical engineering book, for example
Perry's.
Gerard