Tutorial de 
EKO! | Catégories : Outils
The purpose of this tutorial is to make hand-held warmers. These can be heated up to around 50°C when activated, and can be used in the mountains, for example, to keep warm when hiking.
The purpose of this tutorial is to make hand-held warmers. These can be heated up to around 50°C when activated, and can be used in the mountains, for example, to keep warm when hiking.
cuisine, chaleur, chimie, montagne
When we go out in the mountains, we sometimes find ourselves exposed to the cold, particularly on the extremities of the body (hands, feet).
Some people really struggle to keep warm, and ski touring (to avoid the wasteful and not environmentally-friendly ski lifts!) can become a real nightmare!
Some sports shops offer hand-warmers for a little extra comfort. These are small plastic containers that warm up to around 50°C when activated.
Some are reusable, for around 20€ a pair, while others are not, for around 15€ for 30.
In a complete low-tech approach, we should first ask ourselves about this need for comfort. But before we get there, and for those who may already have given this in-depth thought but still feel the need to have warmers, it's possible to make ones by yourself reusable (almost! See the discussion on the problems to be solved) and economical (that, that's confirmed!)!
The quantities will be discussed in the tutorial as they depend on the concentration of the vinegar.
Les compotes à emporter ne conviennent pas toutes, prendre seulement celles qui se rebouchent bien!
Here are the quantities for one warmer ! The mass of vinegar depends on its concentration.
35g baking soda
| Concentration of vinegar [%] | Mass of vinegar [g] | Approximate volume of vinegar [mL] |
| 6 | 415 | 415 |
| 8 | 315 | 315 |
| 10 | 250 | 250 |
| 12 | 210 | 210 |
| 14 | 180 | 180 |
| 16 | 155 | 155 |
These values are approximate. You can find out how to calculate them in the theoretical sections.
NB: The density of vinegar is very close to that of water, 1kg for 1L.
Making warmers involves doing chemistry, and chemistry doesn't take kindly to impurities. We strongly advise you to clean all utensils properly with soap and water. Particularly the containers of the warmers, as there's a risk of a little compote remaining in them if you choose the same ones as us!
Safety
The first step consists of mixing the vinegar and bicarbonate of soda. To do this, start by pouring the right amount of vinegar into the pan. Then add the bicarbonate of soda slowly. Stir until there is no more foam. This indicates that the chemical reaction is complete.
Point of vigilance
Safety
When the first stage is complete, we can put our saucepan on a high heat, the aim being to evaporate all the excess water. I say too much, because we'll need a little more water to get the right substance. When a very light film begins to appear on the surface, then the substance is ready, you need to stop heating.
Point of vigilance
Safety
The aim of this step is to fill the containers of our warmers with the substance obtained in step 4.
Two people are needed for this stage, as it is difficult to hold the containers and pour at the same time.
The person holding the container can wear gloves to limit the risk of burns.
At this stage, a funnel is inserted into the containers and the contents of the saucepan are poured in gently.
Point of vigilance
The warmers are now ready to be loaded!
To charge the warmers with heat, place it in boiling water for 10-15 minutes. Then leave them to cool, without stirring them too much, until they reach room temperature.
They're now full of energy and ready for use in the mountains or anywhere else!
Once you're out in the mountains in the cold, you can activate them by following the instructions.
It then heats up to around 50°C. To keep the heat created, it is advisable to isolate them from the outside air by putting them in your gloves and/or pockets.
Safety
Warning: it is strongly inadvisable to heat up a frostbite suddenly. The use of warmers is preventive, to prevent a strong sensation of cold and not to heat an area in critical condition.
Then, it is not advisable to alternate between hot and cold for frostbite. It's better to wear dry clothes and wait for a bath thermostated at 37°C once you're in a safe place.
It's been very interesting for me to experiment and improve a process following personal observations! I share with you my discoveries from my experiences and my readings.
Sodium ethanoate is a product of the reaction between ethanoic acid and sodium bicarbonate.
Cette réaction produit aussi de l'eau est du CO2.
This part isn't much fun, so skip it if you're not a big fan of chemistry calculations! But it is necessary if you want to recalculate everything yourself!
To determine the quantities of ethanoic acid and sodium bicarbonate to mix, we assume that the reaction is complete. So, in order to optimise everything, we need to mix the reagents in what are known as stoichiometric quantities. When you add exactly these quantities, all the reagents are consumed and all that's left at the end of the reaction is the product!
In our case, one molecule of ethanoic acid reacts with one molecule of sodium bicarbonate. The same number of "quantities of matter" (moles) of each of the two reagents must therefore be added in order to reach the stoichiometric quantities.
Knowing this, calculate the quantity of material corresponding to 35g of bicarbonate (for 1 warmer).
Next, calculate the mass of acetic acid needed to obtain exactly the same quantity of substance (which will depend on its molar mass).
Finally, knowing that, say, 8% vinegar has 0.08g of ethanoic acid per 100mL, we calculate the volume of vinegar to obtain exactly the right mass of ethanoic acid.
If you prefer, you can calculate the mass of vinegar rather than its volume (useful if you don't have a measuring glass). Luckily, vinegar has almost the same density as water, so 1kg of vinegar for 1l of vinegar.
There are a number of educational resources on basic calculations in solution chemistry on the internet if you're interested. This is a subject that is covered at the beginning of secondary school in France.
This reaction is fun to experiment with because it is very visual: the production of gaseous CO2 produces foam. We can then see whether all our molecules have reacted properly.
The reaction takes time, and we have to mix! But what happens in the world of molecules to make it take so long!
In our saucepan, after a few seconds of reaction, we have a lot of water, the reactants and also the few products that have already been created. In order to react, two molecules of reagent must meet.
But how do you meet someone in this mess? It's a bit like throwing pollen into a field of flowers, at first it's easy for the pollen to find a single flower, but after a few minutes, when many couples have formed, it's difficult for a small flower and a pollen to find each other.
In technical terms, we speak of reaction kinetics to refer to the speed at which the reaction takes place and of limiting phenomenon to refer to the phenomenon that imposes this speed.
Here it is the meeting of the molecules that is the slowest, so we speak of mass transfer.
.
We've already discussed the problem of crystallisation if the liquid is heated for too long. This is a rather counter-intuitive observation. Normally, by increasing the temperature, you go from solid to liquid, not the other way round.
The phenomenon of crystallisation comes from the dehydration of sodium ethanoate trihydrate to anhydrous sodium ethanoate. In fact, the trihydrate substance, the one we want for our warmers, liquefies if we heat it above 58°C. On the other hand, the anhydrous substance only liquefies at 324°C. So when you remove the water from a molecule, Bang! It becomes anhydrous and solidifies instantly, because we're well below 324°C!
At the beginning, there's an excess of water, so it's this water that evaporates. But as soon as there is almost no water left, we start to '"dehydrate'" our good old molecule, "'hence the appearance at the end of crystals'", then, progressively '"a solid film'".
Here, knowing the phenomenon allows you to judge when to stop step 4: when the first crystals appear, you know that the remaining liquid is not water but sodium ethanoate trihydrate, because if there was still liquid water, it would evaporate and no crystals would appear!
.
Warmers work on the basis of the phenomenon of supercooling! To find out more, read this article:
In theory, warmers should be reusable. In reality, each time they are used it becomes more difficult to activate them. I haven't been able to solve the mystery of this phenomenon, but maybe you can!
They can be reused a number of times, however, if you are prepared to wait a while and go over them several times to activate them.
For the more persistent, inserting a metal rod and kneading it will activate it more effectively, so you'll be able to reuse it for longer with this method. To do this, you can insert the tip of a small screwdriver, a screw or any metal object, knead it for a while and remove it once the heater starts to heat up :)
Sometimes during recharging, after having warmed them up and once at rest. The warmers may activate by themselves. This can be annoying because you then have to charge them again.
To be sure that a heater is ready to use, simply check that it is liquid. If it is, you're on the safe side.
Fabric pouches enhance the look of the heaters. To hide and hold the compotes: a 20 x 20 cm piece of fabric, hemmed at the top, which is where the compote will enter. Laying out the plastic instruction labels and sewing them at the top and bottom is enough, before sewing the pouch itself on the side and bottom... Looks great...
Noé Beaupere. PILOTAGE DE LA LIBÉRATION DE CHALEUR ET ÉTUDE DU VIEILLISSEMENT DE MATÉRIAUX À CHANGEMENT DE PHASE. Sciences de l’ingénieur [physics]. Université d’Artois, 2019. Français. https://theses.hal.science/tel-03160528
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