Chaufferette/en

Low-tech with Refugees - Low-tech & Réfugiés

https://wiki.lowtechlab.org/wiki/Chaufferette/en

Dernière modification le 02/07/2024

Difficulté

Easy Facile

Durée

1,5 hour(s) heure(s)

Coût

1 EUR (€)

Description

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.

Sommaire

cuisine, chaleur, chimie, montagne

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Introduction

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 environmentally-friendly ski lifts!) can become a real nightmare!

Some sports shops offer hand-heaters 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 heaters, it's possible to make reusable (almost! See the discussion on the problems to be solved) and economical ones yourself (see the discussion on the problems to be solved). It's possible to make your own heaters that are reusable (almost! See discussion on the problems to be solved) and economical (that's confirmed!)!

Matériaux

• Sodium bicarbonate (baking soda)
• Vinegar
• Container for warmers (here empty compotes to take away)

The quantities will be discussed in the tutorial as they depend on the concentration of the vinegar.

Outils

• Saucepan
• Scales
• Spoon
• Funnel
• Glass
• Measuring glass

Étape 1 - Calculating quantities

Here are the quantities for one warmer ! The mass of vinegar depends on its concentration.

Quantity for one warmer

35g baking soda

Concentration of vinegar [%] [g	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.

Étape 2 - Cleaning equipment

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 heaters, as there's a risk of a little compote remaining in them if you choose the same ones as us!

Étape 3 - Mixing reagents

Safety

• Vinegar is irritating to the skin and very irritating to the eyes. Do not hesitate to wear safety goggles when mixing. Otherwise, watch out for splashes.

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

• Pour in the bicarbonate of soda slowly, as the reaction produces CO2 gas, causing the solution to foam.
• This stage takes time, but it's best to get to the end so that all the vinegar reacts. If there is any vinegar left over, be prepared to smell its nauseating odour during the next stage!
• The more warmers you make, the longer the reaction will take. For 5 heaters, you can expect about 20 minutes of mixing.

Étape 4 - Heating, evaporation

Safety

• The substance obtained from the reaction of vinegar and sodium bicarbonate is sodium ethanoate. This substance is irritating, so don't hesitate to wear safety goggles. Otherwise, be careful not to get any in your eyes.
• Slight risk of burns, possible small splashes if large quantities are used on a high-powered hob.

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

• There's a lot of water to evaporate, so this stage takes a while (again, the more heaters you use, the longer it takes to evaporate).
• During this stage, nothing happens for a long time, but in the end everything happens very quickly. You need to be very careful as soon as the liquid becomes slightly cloudy and yellow.
• Generally, crystals will appear on the edges of the pan towards the end.
• If you inadvertently leave the liquid to heat for too long, it will solidify completely. In this case, turn off the heat and add water quickly (not too much, just enough to see all the solid become liquid again). You can then put it back on the heat, stirring to help the last crystals liquefy. Don't worry, the heaters will still work!
• Towards the end, a smell similar to that of a baked cake should appear. It's not unpleasant, but avoid sniffing it too much! It's best to be careful when playing chemist's apprentice! Even when you're handling substances that aren't very dangerous :)

Étape 5 - Filling

Safety

• Risk of burns, as the liquid to be poured into the warmer containers is very hot (around 100°C at first).
• If the liquid comes into contact with the skin at less than 60°C, it will solidify and heat up. It's very impressive because the solid sticks to the skin. Don't panic, a little water and it will go away on its own. However, don't take too long to rinse off with water to avoid burning yourself.

The aim of this step is to fill the containers of our heaters 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

• Leave a small air space in the warmer when pouring in the liquid. Be careful not to completely block the hole with the funnel, as this could cause the liquid to overflow and burn :(
• Between each warmers, stir the pan to mix the liquid and prevent the surface from solidifying.
• The liquid solidifies at around 58°C, so pour it in before it reaches this temperature, otherwise the funnel will be blocked. However, don't pour too quickly or you could get burnt. If the substance starts to cool too much, simply add a little water and repeat step 4.
• If the funnel is completely blocked, you can pour in some hot water and the solid will quickly become liquid and flow!

Étape 6 - Reloading warmers

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!

Étape 7 - Use of warmers

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 heaters 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.

Étape 8 - The theory of warmers

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.

Manufacture of sodium ethanoate, chemical reaction

Sodium ethanoate is a product of the reaction between ethanoic acid and sodium bicarbonate.

This reaction also produces water and CO2.

Calculating quantities

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.

Understanding with your own senses

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.

Why does the reaction (mixing) take so long?

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.

Ici c'est la rencontre des molécules qui est la plus lente, on parle donc de transfert de masse.

Vous avez dit cristallisation ?

On a déjà discuter du problème de cristallisation si on fait chauffer trop longuement le liquide. C'est assez contre-intuitif comme observation. Normalement, en augmentant la température, on passe de solide à liquide pas l'inverse.

Le phénomène de cristallisation provient ici de la déshydratation l'éthanoate de sodium trihydraté vers l'éthanoate de sodium anhydre. En faite, la substance trihydraté, celle que l'on souhaite pour nos chaufferette, se liquéfie si on la chauffe au delà de 58°C. En revanche, la substance anhydre elle ne se liquéfie qu'à 324°C. Ainsi, lorsqu'on enlève son eau à une molécule, PAF ! Elle devient anhydre et se solidifie instantanément car nous ne somme bien en dessous de 324°C !

Au début, il y a de l'eau en excès, donc c'est cette eau la qui s'évapore. Mais dès lors qu'il n'y a presque plus d'eau, on commence à déshydrater nos bonne vieille molécule, d'où l'apparition sur la fin de cristaux, puis, progressivement d'un film solide.

Comprendre pour mieux agir !

Ici, la connaissance du phénomène permet de juger quand arrêter l'étapes 4. En effet, à l'apparition des premiers cristaux, on sait que le liquide restant n'est pas de l'eau mais bien de l'éthanoate de sodium trihydraté, car si il y avait encore de l'eau liquide, c'est elle qui s'évaporerais et aucun cristaux n'apparaitrais !

Le plus important ! Pourquoi les chaufferettes chauffe !

Le fonctionnement des chaufferettes se base sur le phénomène de surfusion ! Pour en savoir plus vous pouvez consulter cette article :

https://ssaft.com/Blog/dotclear/?pages/Acetate-de-Sodium

Étape 9 - Problématique non résolue

Des chaufferettes presque réutilisable !

Les chaufferettes devrait être réutilisable en théorie. Dans la réalité, à chaque nouvelle utilisation il devient plus difficile de les activer. Je n'ai pas su percé le mystère de ce phénomène mais peut être que vous y arriverez !

Elles sont tout de même réutilisable un certain nombre de fois si on accepte d'attendre un peu et de s'y reprendre à plusieurs fois pour les activer.

Pour les plus persistant, en insérant un tige en métal et en la malaxant l'activation est plus efficace donc vous pourrez les réutiliser plus longtemps avec cette méthode. Pour se faire vous pouvez insérer un l'embout d'un petit tourne vis, d'une vis ou tout objet métallique, le malaxer pendant un certain temps et le retirer une fois que la chaufferette se met à chauffer :)

Quelques auto-activations imprévues

Parfois, pendant la recharge, après les avoirs fait chauffer et une fois au repos. Les chaufferettes peuvent s'activer toute seul. Cela peut être embêtant car il faut alors les remettre à charger.

Pour s'assurer qu'une chaufferette est bien prête à utilisation il faut simplement vérifier qu'elle soit bien liquide. Si c'est le cas vous êtes sûr de votre coup.

Notes et références

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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