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1:03
NOW IN ENGLISH: *******www.science-tube**** www****experimente.de chemistry experiments Experiment 115 - fluorescence of various materials part 1 Chemie Versuche - Fluoreszenz verschiedener Materialen Teil 1 Did you enjoy the video? Go to *******www.science-tube**** and watch more of my videos. If you have interst, please contact me for shows, presentations or further education. Also do not hesitate to write me, if you have a question or want to see a new experiment on video.
10 Jul 2007
36532
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0:57
NOW IN ENGLISH: *******www.science-tube**** www****experimente.de chemistry experiments Experiment 119 - Sodium on water part two Chemie Versuche - Natrium auf Wasser 2
10 Jul 2007
36234
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2:13
chemistry experiment
10 Oct 2007
5353
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0:32
If you like explosions, explosives, dry ice bombs, chlorine bombs blowing up your about to be amazed from this simple compound. It should have only been a small fireball....whoops.
1 Feb 2007
43246
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0:17
This has to be one of the best loved show experiment amongst Flensburg’s chemistry students: The wax flame thrower! Since the experiment has found its way into the Flensburg laboratories, it has been shown at a number of events to great acclaim from the audience. This experiment is a relatively safe way to demonstrate combustion. It can also be used in fire safety education. If you try to extinguish burning fat or the wax on the Christmas decorations with water, you get the same effect. This is a serious risk, as your intuition will always tell you to use water to put out a fire. But in these cases, that would be the worst thing to do – as this experiment demonstrates. The combustion you can see so clearly in the video comes about through a number of steps. 1. The test tube is around 400° C hot; exposed to the cold water, it cools down rapidly and the bottom of the tube shatters. 2. Through the hole thus caused, water enters the test tube and meets the hot wax. 3. The water in the test tube evaporates immediately, greatly expands in volume and drives the liquid wax upwards and outwards. 4. The liquid wax and further gaseous components are ejected from the tube and finely disseminated. 5. The heat, fine dissemination and consequent high saturation with Oxygen mean that small, cracked particles (Hydrogen radicals) ignite in the waxen steam. 6. The flame of the radical reaction ignites the liquid part of the wax mixture. So, there is also a lot going on chemically with this experiment. Did you enjoy the video? Go to *******www.science-tube**** and watch more of my videos. If you have interst, please contact me for shows, presentations or further education. Also do not hesitate to write me, if you have a question or want to see a new experiment on video.
10 Jul 2007
4484
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0:36
Dry ice is a fascinating substance which, when handled right, can be the basis for a host of simple experiments. We list many further examples on our web site. But where do you get it from? Big supermarket chains cool their fruit with dry ice. If they are in use, you can see the tubes emitting a cold mist. If you ask at one of these supermarkets, most will let you have some dry ice from their stores. Some supermarkets even offer a free dry ice cooling service when you purchase frozen goods.The dry ice, solid at a temperature of -78° Celsius, evaporates in the much warmer water. Dry ice has the characteristic if changing from a solid state directly to gas. Water can dissolve large amounts of Carbon Dioxide. When saturation is sufficient, a small proportion will react as follows: H2O + CO2 -> H2CO3 The Oxonium ions cause the indicators to change colour. As we did add some alkaline solution, it is more correct to say that this is neutralised first by the Carbonic acid which leads to the formation of small amounts of Carbonate und Hydrogen Carbonate. The soap solution in the first beaker starts to foam as the Carbon Dioxide is released. The white mist is the result of cooling the air, condensing the moisture in the air above the beakers. When using warm water, this is proportionately more intense. Did you enjoy the video? Go to *******www.science-tube**** and watch more of my videos. If you have interst, please contact me for shows, presentations or further education. Also do not hesitate to write me, if you have a question or want to see a new experiment on video.
10 Jul 2007
18043
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0:31
Something we could not do very well without in our kitchens is Baking soda. Baking soda is a baking aid that helps dough to rise, i.e. give more volume to a dough to make it ‚lighter’. This works because Baking soda releases gases that help the dough to rise. The release of such gases works in a number of ways. Carbon Dioxide is released by adding any acidic solution – for baking soda, this is typically achieved by adding citric or tartaric acid in solid form to the baking powder. When adding water, they dissolve and set off the reaction. A second way of achieving the gas release is heat – Baking soda will decompose into gaseous components at a heat of 50° C or more, which is why your cake continues to rise in the oven. The same process is demonstrated in this experiment. The Ethanol begins to burn with a blue flame. The "Emser" cough pastilles become more and more bloated in the heat and take on a black colour. Slowly, longer and longer “worms” emerge. The reaction continues until the alcohol has been burnt off. In addition to their medicinal content, Emser cough pastilles consist of Bicarbonate of soda (baking soda) and sugar. sodiumbicarbonate decomposes from temperatures of 50°C, resulting in Carbon Dioxide and steam. 2 NaHCO3 - > Na2CO3 + CO2 + H2O Reacting in the heat of the alcohol flame, the sugar content of the pastilles is melted and driven into wormlike shapes by the gases provided by the decomposing Baking soda. Did you enjoy the video? Go to *******www.science-tube**** and watch more of my videos. If you have interst, please contact me for shows, presentations or further education. Also do not hesitate to write me, if you have a question or want to see a new experiment on video.
10 Jul 2007
5306
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0:30
Nitric acid is one of the strongest acids in chemistry. Nitric acid is still used today in the mining of Gold as it dissolves common metals very effectively. It even attacks Silver but not Gold – which is why gold is so easily divided from other metals. Gold does not react with Nitric acid. The Magnesium and the Copper shavings react very quickly, releasing a reddish brown gas. The Zinc granules react after a little while in the same way. What is left in the flasks is a solution of the metal salts created by the reaction – the Copper Nitrate solution is green, the Zinc and Magnesium Nitrate solutions are yellow. Nitric acid attacks almost all common and even some of the precious metals, such as Silver and Copper. The only exceptions are the ‘noble’ metals, Gold, Platinum and Iridium. A few other metals, namely Iron, Chrome and Aluminium, are also immune because of their passivation. They form a protective oxidized layer which cannot be dissolved by the acid. Zinc also forms such a layer but it does depend on the distribution of the metal – the finer the dissemination in the acid, the stronger and quicker the reaction. Oxidation: 3 Mg ->3 Mg2+ +6e- Reduktion: 2 NO3- + 8H3O+ + 6e- -> 2 NO + 12 H2O 3 Mg + 2 NO3- + 8 H3O+ -> 3 Mg2+ 2NO + 12 H2O The released Nitrogen Monoxide is colourless but reacts immediately with the Oxygen to form brown Nitrogen Oxide. 2 NO (uncoloured) + O2 -> 2 NO2 (brown)
10 Jul 2007
13128
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0:09
An Experiment on the the Chemistry Course. An Ballon filled with hydrogen explode. Kemi Experiment
15 Jan 2008
1577
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3:34
For the HSC Chemistry syllabus dot-points: “Perform a first-hand investigation to prepare and test a natural indicator” and Solve problems by applying information about the colour changes of indicators to classify some household substances as acidic, neutral or basic”. We crushed some red cabbage immersed in ethanol to extract the anthocyanin. This purple solution was applied to several household solutions varying in pH and the range of colours were analysed according to the known acidity / basicity of the solutions tested.
2 May 2011
664
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6:34
Part 1 of 2. For the HSC Chemistry syllabus dot-point: “Perform a first-hand investigation and solve problems using titrations including the preparation of standard solutions, and use available evidence to quantitatively and qualitatively describe the reaction between selected acids and bases”. This experiment is important because it is one of the most commonly chosen experiments for Prac Exams. Prac Exams could come any time throughout year 12 – but most of the time they occur as part of your trial HSC exams, and usually worth around 20% of total internal assessment. Therefore it is important to pay close attention to proper titration procedure and understand the underlying processes of neutralization reactions. For this titration, our unknown was a solution of NaOH (the analyte) and our standard solution was oxalic acid (crystals in dihydrate form) – the titrant. Glassware was rinsed properly with either deionised water or with the solution it was to contain (conical flask, volumetric flask – water / pipette, burette – solution). A total of 1 ‘rough titre’ and 3 accurate titres were done. The average of the 3 accurate titres were recorded and used to finally calculate the concentration of the unknown NaOH. Our indicator was phenolphthalein due to its slightly basic endpoint (the titration was between a strong base and a weak acid, therefore the equivalence point would be slightly basic). Tip: If required to make your own standard solution, make sure you design your standard solution so that it was enough moles for you to do 3 titres.
2 May 2011
1208
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2:06
Apparently thanks to automatic sprinklers people cannot even conduct a cool experiment involving fire. The whole classroom was drenched.
2 Oct 2018
589
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