A list of experiments, in order:
- Manganese Heptoxide
The first few videos are of chemicals being oxidized by manganese heptoxide. At first the sulfuric acid reacts to form permanganic acid but the dehydrating nature of sulfuric acid causes manganese heptoxide to form, according to this reaction:
2KMnO4 + 2H2SO4 --> Mn2O7 + H2O + 2KHSO4
It completely oxidizes ethanol, sulfur, citric acid, and the fats and oils in a potato chip, while reducing itself to the brown MnO2 soot that is observed.
- Chlorine and Acetylene
In the next set of experiments, chlorine gas and acetylene gas react. The standard equation for this is C2H2 + Cl2 --> 2C + 2HCl; however, unsaturated and saturated forms of chlorinated 2 carbon organic structures are produced as side products as well. This includes molecules such as C2H2Cl2 and probably C2H2Cl4. More information can be found on woelen's page
- Chlorine and Turpentine
Chlorine reacts with turpentine in a similar reaction. Once again a hydrocarbon reacts to form HCl and carbon, and likewise the formation of chloriniated organic compounts is possible.
C10H16 (l) + 8Cl2 (g) --> 16HCl (g) + 10C(s)
- Sugar and Potassium Chlorate
Next, sugar is burned with potassium chlorate. This is the same reaction as the classic demonstration where a gummy bear is dropped in molten potassium chlorate. Potassium chlorate is reduced to potassium chloride and oxygen, while sugar is burned to form a variety of products including carbon dioxide and carbon.
- Suagr and Sodium Chlorite
Sugar will reduce even more violently with sodium chlorite. The oxyhalide anions become less stable the less oxygens that are bonded due to stability of the structure of the ion, this is shown here and in the next demonstration.
- Vitamin C and Sodium Chlorite
Vitamin C is a reducing agent, and sodium chlorite need only be stirred with vitamin C to be reduced in flames. A small green hue is observed slightly before ignition; this is likely chlorine gas as a decomposition product of sodium chlorite, despite that the standard equation for the decomposition of sodium chlorite is
NaClO2 --> + NaCl + O2
- Aluminum and iodine
In the reaction between aluminum and iodine, aluminum iodide is formed. This reaction is very exothermic however, and is able to sublimate some of the volatile iodine. The result is a thick smoke containing aluminum iodide and iodine.
- Zinc, Ammonium Nitrate, and Sodium Chloride
In the mixture of zinc, ammonium nitrate, and sodium chloride, the chloride ion is key. A mixture of ammonium nitrate and zinc can be ignited with a drop of hydrochloric acid. Once lit, the zinc is burned and the ammonium nitrate provides the oxygen.
- Nitrile gloves and Red Fuming Nitric Acid
Not much information can be found on the reaction between red fuming nitric acid and nitrile, however it is well known that nitrile is subject to acid hydrolysis. This reaction does not work with anything less the red fuming nitric acid however, so the strong oxidizing properties of RFNA are important.
- Magnesium Silicide in Hydrochloric Acid
When magnesium silicide and sand are heated with a torch in a test tube, two reactions occur. First, the sand (silicon dioxide) has its oxygens removed by the magnesium, forming magnesium oxide according to the following reaction:
SiO2 + 2Mg --> Si + 2MgO
Extra magnesium in the test tube reacts with the silicon to form magnesium silicide.
2Mg + Si -> Mg2Si
The top of the mixture in the test tube must be covered with sand while heating to prevent the magnesium from burning. When the magnesium silicide is introduced to acid, the magnesium goes into solution as a 2+ ion while the silicon reacts with the hydrogen ions to form silane gas, SH4:
Mg2Si(s) + 4H+(aq) --> Mg2+(aq) + SiH4(g)
More information can be found here.
- Potassium Permanganate and Glycerin
Potassium permanganate will start a fire when mixed with a variety of organic material; most famous is glycerin, for its use in starting thermite reactions. The equation is a follows: 14KMnO4 + 4C3H5(OH)3 --> 7K2CO3 + 7Mn2O3 + 5CO2 + 16H2O.
- Magnesium and Silver Nitrate
In solution, magnesium and silver nitrate will react to precipitate silver and form magnesium nitrate. This reaction is exothermic however. When dry magnesium and silver nitrate are mixed, this reaction begins when a small amount of water is added. This reaction is hot enough to decompose the silver nitrate and burn the magnesium. Rather than mixing the dry powders and adding water, which is extremely dangerous, the silver nitrate was made already wet so the reaction time could be better predicted.
- Chlorine induced flash
For the chlorine induced flash, aluminum reacts with potassium nitrate according to: 6KNO3 + 10Al --> 3K2O + 3N2 + 5Al2O3. The phosphorus is there for ignition, but also reacts with the potassium nitrate according to: 6KNO3 + 6P --> 2K3PO4 + 3N2 + P4O10.
More information here.
- Periodic Acid and Phosphorus
Anhydrous periodic acid comes in two forms, orthoperiodic acid, H5IO6, and, when dehydrated, metaperiodic acid, HIO4. In this demonstration orthoperiodic acid, which is a strong oxidizing agent, has red phosphorus poured onto it. More information here.
- Periodic Acid and Hydrazine
Periodic acid reacts with an ever more powerful reducing agent, hydrazine hydrate. Anhydrous hydrazine was used as a hypergolic liquid rocket fuel with inhibited red fuming nitric acid in the past. Here, a 20% solution of hydrazine hydrate is used instead and still reacts incredibly with periodic acid.
- Phosphine and Chlorine
White phosphorus, prepared by the micro distillation of red phosphorus, reacts with hot concentrated hydroxide solution deadly phosphine gas is made, as well as the hypophosphite ion:
P4 + 3OH– + 3H2O --> PH3 + 3H2PO2–
Due to this side reaction however, this gas would burst into flames on contact with air:
3P4 + 8OH– + 8H2O --> 2P2H4 + 8H2PO2–
The P2H4 side product, diphosphane, is pyrophoric.
When the main product of phosphine encounters chlorine, the following reaction occurs:
PH3 + 3Cl2 --> PCl3 + 3HCl
Both products are soluble in water.
- Nitromethane and Sodium Oxide
The last reaction is a take on the classic yet complex reaction between sodium hydroxide and nitromethane. Many products are formed, resulting in a brown residue. This reaction is more violent however, when sodium oxide is used instead, and leads to instant flames.
More information