Department of Energy Argonne National Laboratory Office of Science NEWTON's Homepage NEWTON's Homepage
NEWTON, Ask A Scientist!
NEWTON Home Page NEWTON Teachers Visit Our Archives Ask A Question How To Ask A Question Question of the Week Our Expert Scientists Volunteer at NEWTON! Frequently Asked Questions Referencing NEWTON About NEWTON About Ask A Scientist Education At Argonne Fill and Evaporation Rates
Name: Robert
Status: Educator
Grade: 9-12
Location: WA
Country: United States
Date: December 2007


Question:
Hi, I am an Engineer at HP but I am volunteering at my son's high school. I would like to structure a problem for the students which would include a liquid substance that is 80% water going into a container subject to evaporation. The question is: How long would it take to fill a container of X mm if the liquid goes in at a specific rate given an vaporation rate (of course there will be some precipitate remaining after full evaporation)? What I would like to do is then have the students construct an experiment to accelerate that behavior (at elevated temp and low humidity) but I think I would need to do this at ambient first so I could get an acceleration factor. Ideally, it would be great if I could have a formula that equates volume as a function of time and temperature. I thought I could use elementary differential equations for this but it may actually be simpler than that. Any thoughts?



Replies:
I will guess there is probably a simpler way. The evaporation rate depends on surface area, so if you are filling a cylindrical container, you may be able simply to subtract a constant evaporation rate from the fill rate to get the net fill rate.

If the evaporation rate also depends on the concentration of whatever substance represents the other 20% of the liquid going in, then you will need a differential equation. I will guess the evaporation rate will depend on the fraction of molecules at the surface that are water, so once the concentration has increased to the point that a precipitate is being formed, the surface fraction will stop changing, and you'll be back to simple subtraction.

Tim Mooney


We frequently receive inquiries about "rates" of evaporation in one form on another. The problem is that "rates" of [evaporation, crystallization, condensation, ...] the list is long are very difficult to measure reproducibly because important variables (such as relative humidity) are difficult to control. Example: if the relative humidity of the air is 100% it does not matter how fast you blow air across a sample, no water will evaporate, so the solution will always become water-enriched. In turn, the relative humidity is a sensitive function of the temperature of the aqueous solution, and there is a "feedback" mechanism since the preferential evaporation of some volatile component -- say acetone -- alters the partial pressure of water, and the evaporation causes a reduction of the temperature solution which changes the values of all of the above. All of these (and other) variables have "feed back" on the conditions of evaporation.

While it may be an oversimplification, this is why it is very difficult to predict weather. There are so many "feedback" variables operating I fear that the differential equations will be non-linear. Way too involved even for "state of the art" experts. Sorry, wish it were simpler.

Vince Calder


Robert,

You can make this situation somewhat simple, or you can make it quite complicated. The more precise you want to be -- and I am not sure how precise you would need to be for the exercise to be reasonably accurate (valuable?) -- the more complicated. I am going to try to give you some considerations, and you can decide (with experimental data) which can be safely neglected. I am also going to give you the names of certain equations, but since you are comfortable with differential equations, I am going to assume you can find them and solve them -- but please feel free to email me back if you want help with those steps.

First, you stated you want the container to have a liquid that is 80% water. What do you want the other 20% to be? If you choose a soluble solid -- e.g. sugar or salt for instance -- that would not evaporate, then you can approximate the partial pressure exerted by the water using Raolt's law (the mole fraction of the water times its partial pressure). When you know the partial pressure of the water at its surface, you can make some simplifying assumptions to calculate the mass transfer. For instance, assume you have a cylindrical container and that the partial pressure of water at the exit (top) of the container is ambient humidity. The partial pressure is a function of temperature. You can then estimate the mass transfer of water by diffusion from the surface to the top of the container by Fick's Law (diffusion also is a function of temperature). If you are filling the vessel, or waiting a long enough time that the length of the vapor column (from the surface to the container top) changes, then the equations become more challenging to solve analytically. Likewise, if you wait a long time, the water will become depleted, its mole fraction will drop, and thus you have another variable in your equations instead of a constant. I would recommend a math software package such as Mathcad to solve them numerically.

If you want the other 20% to be a volatile liquid, such as ethanol, methanol, etc. Now you have a different situation. Here you have a binary mixture in equilibrium with the airspace above it. Each liquid exerts a partial pressure that is a function of the mole fraction of each liquid, also according to Raolt's law. I recommend you find what's called a T-XY diagram for the mixture you select -- it tells you the vapor equilibrium concentration at a given temperature and liquid composition. You can then repeat the procedure above -- but if you run the experiment for a long enough period of time, you are going to have the mole fractions of each liquid changing along with the level of the fluid -- again, begging for a numerical solution.

Both of these discussions neglect convection, and assume well-mixed liquids. Neither may be true -- you could have depletion of more volatile substances at the surface of the liquid (especially in the case of the sugar solution, as its viscosity would inhibit mixing), and you could have convection currents in the vapor phase causing higher mass transfer than diffusion alone would predict. Especially if you are elevating temperature, these convection currents would be more likely to develop. Also, as the liquid evaporates, it carries energy with it. Water has a high heat of vaporization, which means water that is left out to evaporate will be cooler than ambient. This will affect the partial pressure at its surface as well as diffusion.

So in summary, you have several conditions that are changing: the mole fraction of each component, the level of the liquid, the temperature -- which affects the partial pressure of each component and the diffusion coefficients of each component, and keeping in mind that the temperature at the surface of the liquid will be lower than ambient. Very complicated, and I'm not sure if all this complication is even useful, so I'm going to start from the other side -- the experiment.

Let us start with pure water in a partially full cylindrical tube. Let us try to model its evaporation. At the surface we have a partial pressure (a function of temperature), and we assume ambient humidity at the exit of the tube. Given Fick's law, we can find flux and with the cross sectional area, mass transfer. You can then calculate an instantaneous volume change. As the volume level drops, the distance through which evaporation occurs increases, which decreases the mass transfer. So as the water evaporates, the rate of evaporation slows down. Neglect everything else for the time being. Does this data match your experiments where you leave out the tube for some period of time? If yes, then you are done. If not, add in other variables until you get the precision you desire. Go ahead and change your temperature and humidity with this single-component case too if you like.

Now, add in your second component and repeat the above experiments. Again, keep adding in variables until you get the desired precision. Which variables? Try the ones that are easiest to measure. If you have a temperature probe, stick it in the water. Compare it to the air temp. Have a video camera? Record the evaporation over time, and gather very precise data on the liquid level. These are just two examples.

Alright, I guess this has gotten long-winded enough. I hope I have given you some food for thought in designing your experiment.

Burr Zimmerman


I agree with Vince Calder that this is a very difficult experiment to control very precisely. However, this is an opportunity to make a try, see how it works, and refine from there. Hey, this is what experimental science is all about!

Vince Calder alludes to a very tricky variable called 'latent heat of vaporization' -- which is the energy it takes to vaporize a substance that is already at its vaporization temperature (there is also a latent heat of fusion, the energy to go from liquid to solid) to vaporize. This is relevant to this discussion because the water at the surface will be *colder* than ambient because as it evaporates, it cools (the vaporized water takes heat with it). If you have ever drank chilled water from a terra cotta water jug, you have seen this effect in action. The porous terra cotta allows some water to pass though it and evaporate, chilling the remaining water. I heard somewhere that Indians (from India -- not Native Americans) actually used the same effect to make ice. It is the same reason damp clothes feel 'cool' -- water is evaporating. Anyway, this is a very difficult thing to control -- or to measure -- so it is something to keep in mind.

The reason this effect is important for you is that the vapor pressure of the liquid is a function of temperature, and if your liquid is not well-mixed, you will get less evaporation than you think because the surface is cooler than ambient. Even in a temperature-controlled chamber, the temperature at the liquid surface may be quite different than you expect.

Another variable you discussed was a mixture of two substances. You did not say whether you meant two liquids, or one liquid and one solid. However, both will affect evaporation rates. I will not go into too much detail here -- but please reply if you require more info -- but I would point you to 'Raolt's Law' to begin. As the more volatile liquid evaporates the remaining substance will concentrate, and the rate of evaporation will change. Calculating accurately with so many changing variables is very difficult to do.

I can offer you a suggestion -- but please adjust for your own circumstances. The goal is to create a setup that makes calculations easier. With simpler calculations, you have an easier time matching up your results with your calculations. I would use a very tall, narrow vessel (like a clear plastic tube) with an aspect ratio of 10 or higher -- depends on the size of your chamber. I would seal the bottom, fill with a small amount of water (~1 diameter in depth). I would put a magnetic mixing bar in the bottom to keep the water well mixed -- make sure you do not turn up so high that it forms a vortex. I would use deionized water to reduce the effect of solutes on the evaporation rate.

The reason you want the water well mixed is to ensure it is at the same temperature throughout instead of developing the cold surface as previously mentioned -- as best as you can at least. The mixing bar will add some heat as well, which may counteract the enthalpy of vaporization. The long head space is to set up an unmixed diffusion column, which will minimize the effect of wind or drafts. You can assume that the concentration of water vapor at the liquid surface is the partial pressure of water at the ambient temperature. You can assume the partial pressure at the top is the ambient humidity. You can then calculate diffusion of water in air through the length of the column (adjusting for the fact the column gets larger as the water evaporates). Using Fick's law, you can calculate the flux of water through the column, and then compare to experimental results. If you have some probe thermistors, you could also mount one each near the surface and near the bottom and measure water temperature directly instead of assuming it is at ambient (be sure to calibrate each). If you need help with any of the calculations, please let me know. Since you said you are comfortable with differential equations, you may be able to do these without any problem.

As for different runs, I would *not* hold one constant while you vary the other. It is better to pick a set of conditions that span all variables' ranges. This is known as 'design of experiments' -- you get higher quality data this way -- and can do so running fewer experiments. For instance, if you have temperatures A, B, and C and humidities 1, 2, and 3, you could run 9 experiments -- A1 A2 A3 B1 B2 B3 C1 C2 C3. That is known as a full factorial. You can run subsets of that too depending on your time budget. If you picked one level to hold for each variable, you might pick 2 and B -- and run A2, B2, and C2, and then B1 and B3. That is five experiments. However, for 5 experiments, you may get better data running A1, C3, A3, C1, and B2. If the effects at the extremes are more important to know, this may be better. As you get into more complex experiments, with many more variables, techniques such as this become critical to get the most out of your experiments. If you want help with this aspect, let me know, but I would suggest you Google things like experimental design and full factorial / fractional factorial, Box Behnken, central composite, Placket-Burman. Experimental design is a HUGE field though, so be warned! (it is really interesting and useful too though). I just came across this site which seems good at first glance:

http://www.itl.nist.gov/div898/handbook/pri/pri.htm, so maybe look at it.

Hope this helps,
Burr Zimmerman



Click here to return to the Engineering Archives

NEWTON is an electronic community for Science, Math, and Computer Science K-12 Educators, sponsored and operated by Argonne National Laboratory's Educational Programs, Andrew Skipor, Ph.D., Head of Educational Programs.

For assistance with NEWTON contact a System Operator (help@newton.dep.anl.gov), or at Argonne's Educational Programs

NEWTON AND ASK A SCIENTIST
Educational Programs
Building 360
9700 S. Cass Ave.
Argonne, Illinois
60439-4845, USA
Update: June 2012
Weclome To Newton

Argonne National Laboratory