Experiments with gases. Fun chemistry experiments at home

ENTERTAINING EXPERIENCES AT HOME
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Experiments with gases. Chemical experiments

Entertaining experiments in chemistry

Entertaining experiences at home / Chemistry experiments for children

To work with gases, first of all, we will need plugs with holes and gas outlet pipes.

The tube can be glass, metal or even plastic. It is better not to take a rubber cork - it is difficult to drill holes in it. Take cork or polyethylene stoppers - holes in them can be burned with a heated awl. Insert a tube into this hole - for example, from an eyedropper; it should enter the cork hole tightly, without gaps, so the hole in the cork must first be made slightly smaller than required, and then gradually expand it, fitting it to the diameter of the tube. Put on a glass tube a rubber or polyethylene flexible tube 30 centimeters long, also insert a short glass tube into its other end.

Now the first experience with gases. Prepare lime water by pouring hot water (1/2 cup) over half a teaspoon of crushed slaked lime, stir the mixture and let stand. A transparent precipitate over the settled solution is lime water. Carefully drain the liquid from the sediment; this laboratory technique, as you remember, is called decantation.

If you do not have slaked lime Ca (OH)₂, then lime water can be prepared from two solutions sold in a pharmacy: calcium chloride CaCl₂ and ammonia NH₄OH (aqueous ammonia solution). When mixed together, clear lime water is also obtained.

Grab a chilled bottle of mineral water or lemonade. Open the cork, quickly insert the cork with the gas outlet tube into the neck, and lower its other end into a glass of lime water. Place the bottle in warm water. Gas bubbles will come out of it. It's carbon dioxide CO₂ (aka carbon dioxide, carbon dioxide). It is added to water to make it tastier.

The gas enters the glass through the tube, it passes through lime water and it becomes cloudy before our eyes, because the calcium hydroxide contained in it turns into calcium carbonate CaCO₃, and it is poorly soluble in water and forms a white turbidity.

To experiment with lime water, it is not necessary to buy lemonade or mineral water. After all, when we breathe, we consume oxygen and release carbon dioxide, the same gas that makes lime water cloudy. Dip the end of any clean tube into a fresh portion of lime water and exhale through the tube several times - the result will not be long in coming.

Open another bottle, insert a stopper with a tube and continue to pass carbon dioxide through the lime water. After some time, the solution will become clear again, because carbon dioxide reacts with calcium carbonate, turning it into another bicarbonate salt, Ca(HCO₃)₂, and this salt just dissolves very well in water.

The next gas we'll be looking at has been mentioned quite recently: ammonia. It is easy to recognize by its sharp characteristic smell - the smell of pharmaceutical ammonia.

Pour some boiled saturated washing soda solution into the bottle. Then add ammonia, insert a stopper with a flexible outlet tube into the neck and put the test tube upside down on its other end. Warm the bottle in warm water. Ammonia vapor is lighter than air and will soon fill an inverted test tube. Still holding the tube upside down, carefully lower it into the beaker of water. Almost immediately, the water will begin to rise up into the test tube, because ammonia is highly soluble in water, making room for it in the test tube.

At the same time, you can learn to recognize ammonia - and not just by smell. First, make sure the ammonia solution is alkaline (use phenolphthalein or homemade indicators). And secondly, conduct a qualitative reaction for ammonia. A qualitative reaction is one that allows you to accurately identify a particular substance or group of substances.

Prepare a weak solution of copper sulphate (it should be pale blue) and lower the gas outlet tube into it. When will ammonia begin to be released?₃, then the solution will turn bright blue at the end of the tube. Ammonia with a copper salt gives a brightly colored complex compound of a rather complex composition [Cu(NH₃)₄]SO₄.

Now try to get a very small piece of calcium carbide - we will get acetylene. Assemble the device, as in the previous experiment, only pour not ammonia into the bottle, but soda. Dip a small, pea-sized piece of calcium carbide, carefully wrapped in blotting paper, into it and insert a cork with a tube. When the blotting paper gets wet, gas will begin to be released, which you will collect in an inverted test tube as before. After a minute, turn the test tube upside down and bring a lit match. The gas will ignite and burn with a smoky flame. This is the same acetylene that gas welders use.

By the way, not only acetylene is obtained in this experiment. An aqueous solution of calcium hydroxide, i.e. lime water, remains in the bottle. It can be used for experiments with carbon dioxide.

The next experiment with gases can be done only with good ventilation, and if it is not, then in the fresh air. We will get a strong-smelling sulfur dioxide (sulphurous gas) SO₂.

Pour dilute acetic acid into a bottle and add some Na sulfite wrapped in blotting paper.₂SO₃ (This substance is sold in photo shops). Close the bottle with a cork, lower the free end of the gas outlet tube into a glass with a pre-prepared dilute solution of potassium permanganate KMnO₄ (this substance is known in everyday life under the name of potassium permanganate). The solution should be pale pink. When the paper gets wet, sulfur dioxide will start to come out of the bottle. It reacts with potassium permanganate solution and discolors it.

If you can't buy sodium sulfite, then replace it with the contents of a large cartridge of a conventional photodeveloper. True, in this case there will be an admixture of carbon dioxide in sulfur dioxide, but this will not interfere with the experiment.

Author: Olgin O.M.

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