Finding Henry's Law Constant for Water Vapor & Sulfuric Acid

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Discussion Overview

The discussion centers around finding Henry's law constant for water vapor in the context of its absorption into sulfuric acid. Participants explore the implications of this constant for drawing equilibrium curves and operating lines in a gas-phase controlled system, considering factors such as temperature, pressure, and concentration.

Discussion Character

  • Exploratory
  • Technical explanation
  • Mathematical reasoning
  • Debate/contested

Main Points Raised

  • One participant seeks to determine the appropriate Henry's law constant for water vapor in sulfuric acid absorption, noting the need for values at various temperatures and pressures.
  • Another participant clarifies that the equation y*=Hx represents a line, not a curve, and suggests using equilibrium data for concentrated solutions.
  • Some participants discuss the relationship between the operating line and equilibrium line, with questions about whether they can be the same under certain conditions.
  • There is mention of using the Kremser Equation to find Henry's coefficient if the solute is assumed to be dilute.
  • One participant expresses uncertainty about how to construct the equilibrium line and whether their current graph accurately represents both lines.
  • Concerns are raised about the availability of equilibrium data and whether it should be specifically for water vapor, given the gas-phase control of the system.
  • Another participant suggests that obtaining equilibrium data directly would be more straightforward than calculating Henry's law constant through assumptions.

Areas of Agreement / Disagreement

Participants do not reach consensus on the best approach to find Henry's law constant or the construction of the equilibrium curve. Multiple views on the relationship between operating and equilibrium lines are presented, and uncertainty remains regarding the necessary equilibrium data.

Contextual Notes

Participants mention various assumptions, such as the solute being dilute and the need for specific equilibrium data, which may affect the calculations and conclusions drawn. The discussion also highlights the complexity of the system and the potential for different interpretations of the data.

moleman1985
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I need to draw an equilibrium curve for a process the equation being
y*=F(x)
y*=Hx, where H is henry's coefficient or constant, but I carnt find H and do not know which H I need (for which substance).
It is for the absorption of vapour water into sulfuric acid so I think I need to find the Henry's value for the water vapour and preferably at different temperatures and different pressures, the system is gas phased controlled.

thankyou
 
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moleman1985 said:
I need to draw an equilibrium curve for a process the equation being
y*=F(x)
y*=Hx, where H is henry's coefficient or constant, but I carnt find H and do not know which H I need (for which substance).
It is for the absorption of vapour water into sulfuric acid so I think I need to find the Henry's value for the water vapour and preferably at different temperatures and different pressures, the system is gas phased controlled.

thankyou

Hello, this is my first post here and I have to improve my English level, so sorry if I can't answer clearly your question.

Firstly, If you say that you want to draw an equilibrium curve.

The expresion y*=Hx, it's not a curve. It is a line. Usually if we work with a not concentrate solutions we can use the expresión because the equilibrium curve is like a line, and if you want to estimate the stages with McAbe-Thiele for the absorption it will be easy.

Then, if the solution is high concentrated you have to use a table with the sulfuric acid-water data, because the equilibrium will be a curve. In this case, if you want to aply McAbe-Thiele method you can work with a "soluto free basis" to transform your curve in a line.

The values you need are the equilibrium values for the Sulfuric acid - water system.
 
hi yes it is a dilute solute, I have all the mole fractions in and out of the absorption system and have drawn an operating line, is this operating line also infact the equilibrium line? I understand that this operating line gives me, y and x values (the solute fraction in the gas and liquid), but what else can I possible get from this line. Thankyou.
 
If I understand you correctly, the line you have dranw is the Equilibrium Line,
to draw the operation line you have to aply this equation:

G(Y1 - Y) = Ls(X1 - X)

being 1 the bottom of the tower.

Anyway you can obtain the same line joining the points (X1,Y1) [ bottom ] and (X2,Y2) [top] :smile:
 
Last edited:
ah yes that what my lecturer was saying to me, but if I presume that the mass transfer throughout the column is constant, won't the equilibrium line also be the operating line?
 
moleman1985 said:
ah yes that what my lecturer was saying to me, but if I presume that the mass transfer throughout the column is constant, won't the equilibrium line also be the operating line?

If the operation line is also the equilibrium line, your tower have no stages and this never happens.
( To explain that clearly you can see this graphic. The stages are calculated always between the two lines )

If you think about you have said, you'll see that you have calculated the operation line to specific concentration in the top, usuallý defined by performance. If you change the performance of the tower, the points (x1,Y1) (x2,Y2) will be diferent , and the operation line too.
 

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Think I understand but that graph shows a straight line for the operating line which I have already, and a curve for the equilibrium line, I know how to extrapolate data from the two lines but cannot draw an equilibrium line I think. I constructed my operating line using (y1,x1) and (y2,x2) or should that be my operating line, if so how do I construct the other line.
thankyou.
 
Could you copy here the wording of the absorption , and the dates you have to resolve it ?

Maybe this way I can resolve your problem. Thanks.
 
hello after doing some further calculations I have obtained this graph which I hope shows an operating line and a equilibrium line, it looks like it.
The operating line is the straight one and was drawn using (x1,y1) (x2,y2), just those two points and they were joined and think has a gradient of approx. L/G.
The curve I hope is the equilibrium line, I constructed this by spliting the column into 10 equal stages, and presumed a constant mass transfer rate, the begging and end point are also (x1,y1) (x2,y2), but has the intermediate sections in it too.

Would this be correct? thankyou.
 
  • #10
graph op. vs. eq.?

sorry this is the graph i drew
 

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  • #11
Hi, he looks good to me a priori.

My first option to draw the equilibrium line is taking real equilibrium dates, no spliting the tower, because the most important reason to do the operating line- equilibrium lin graphic is to obtain the real stages of the tower, but if they don't give you equilibrium dates, table or Henry's constant you can't do in another way.

Cheers.
 
  • #12
I need to draw an equilibrium curve for a process the equation being
y*=F(x)
y*=Hx, where H is henry's coefficient or constant, but I carnt find H and do not know which H I need (for which substance).
It is for the absorption of vapour water into sulfuric acid so I think I need to find the Henry's value for the water vapour and preferably at different temperatures and different pressures, the system is gas phased controlled.

thankyou

If you assume that the solute is dilute, then you can find the henry's coefficient using the Kremser Equation, if you set up your operating line in the solvent free basis.
 
  • #13
siddharth said:
If you assume that the solute is dilute, then you can find the henry's coefficient using the Kremser Equation, if you set up your operating line in the solvent free basis.

The kremser equation for how many stages ? 10 ? It's not a date, it's assumption.
 
  • #14
daysyworld said:
The kremser equation for how many stages ? 10 ? It's not a date, it's assumption.

Yes, you're right, didn't notice that.

I suggest that the OP posts the question in full, exactly as it was given to him/her.
 
  • #15
I've tried to find data to draw an equilibrium curve but cannot find it although that doesn't mean its not out there. The absorption tower consists of a gas stream containing water vapour and it needs to be reduced, the solvent used is 98% wt sulfuric acid, the acid at the bottom becomes 75% wt, due to its absorption.
So if I was to get equilibrium data would I have to get it for water vapour? as I am presuming that it is gas phase driven.
So was I wrong about my equilibrium curve then?
 
  • #16
moleman1985 said:
I've tried to find data to draw an equilibrium curve but cannot find it although that doesn't mean its not out there. The absorption tower consists of a gas stream containing water vapour and it needs to be reduced, the solvent used is 98% wt sulfuric acid, the acid at the bottom becomes 75% wt, due to its absorption.

Do you know the number of stages?
 
  • #17
No i don't know the stages, I thought I could get that off the graph if I ever get an equilibrium line.
All I have to go off is the compositions of the liquid and gas in and out, everything else I have to do, although I know I have to use packed tower and plates, and a mid-way recycle which is cooled.
 
  • #18
moleman1985 said:
No i don't know the stages, I thought I could get that off the graph if I ever get an equilibrium line.
All I have to go off is the compositions of the liquid and gas in and out, everything else I have to do, although I know I have to use packed tower and plates, and a mid-way recycle which is cooled.

In that case, as daysyworld pointed out, I don't think you can find it.

Anyway, why do you want to calculate the Henry's law constant this way :confused: ? It's actually much easier to separately get the equilibrium data for this system at the given temperature and pressure. For example, look up a chemical engineering handbook.
 
  • #19
so I'm presuming that because its gas phased controlled I would just need to find equilibrium data for water vapour at the given pressure and temperature?
my pressure is just atm. but there will be some pressure loss will this have to be considered in the calculations or would it be ok to presume atm. pressure all over.
Thankyou.
 
  • #20
I have perry's so should have the data needed, but I cannot find it anywhere I have been trying for weeks and weeks to get this data, I just need to know how to draw an equilibrium curve (x,y) for my system.
The gas stream in has water that needs to be removed, it is a dilute stream, the solvent used is sulfuric acid it comes in at 98% wt. and out at 75% wt.

So to get an equilibrium curve a presume I'll need the following which I have.
The x and y values in and in of the column, the temperature, and the pressure.

I don't know, the number of stages.

How can I draw an equilibrium line from this data.

Thankyou.
 

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