UVKCHEM is a private non-school and non-corporate entity that carries out independent chemical research. Our main area of expertise is in the electrochemical fields, whereby electrolysis is the main focus.

A. Generation of Hydrogen for use as a fuel.

Hydrogen gas is readily prepared by electrolysis of dilute sulfuric acid utilizing platinum coated electrodes.

Simple setup for electrolyzing dilute sulfuric and to form hydrogen gas. Oxygen gas is a secondary product.

Experimental apparatus for generating hydrogen gas. A ice bath is used to chill the reaction flask (not illustrated).

B. Generation of Oxygen to fix the atmosphere of earth and Mars.

Oxygen is generated by electrolyzing dilute sulfuric acid in the presence of sodium bisulfate utilizing platinum electrodes. The oxygen gas is then collected by displacement under vacuum.

This apparatus is preferably made of nickel steel, and is used to decompose iron oxide into oxygen and molten iron. The molten iron is drained-off through the bottom, and the oxygen is vented via the vacuum manifold. The apparatus is heated in a magnetic field using an appropriate machine (not illustrated).

In series, electro chemical reaction asetup for generating hydrogen and oxygen gasses for atmospheric fixation.

C. The experimental field to generate chemical gases for chemical reactions.

A gas mixture of hydrogen and oxygen is produced by electrolyzing a mixture of sulfuric acid and sodium hydrogen phosphate utilizing platinum coated steel electrodes. An intermediate of potassium permanganate and potassium bifluoride is used to speedup the reaction. A mixture of hydrogen fluoride is produced which is recycled back to the system by means of a condenser pictured above.

Apparatus for generating a fluorine containing oxide gas, containing free chlorine radicals.

Apparatus for generating a fluorine containing oxide.

Electrochemical apparatus for generating ozone gas by electrolyzing a mixture of hydrogen peroxide, potassium perchlorate, and sodium amide.

D. General electrochemical reactions/processes.

Apparatus for production of chlorates, mainly sodium, potassium, and lithium chlorates. The corresponding sodium, potassium, or lithium chloride salts are dissolved in distilled water to form a brine solution. A little potassium dichromate is then added, and the cell is then powered up to about 50 volt at 6 amp. This brine solution is then electrolyzed, whereby chlorine gas is generated in the anode compartment. This chlorine gas is then bubbled directly into the cathode compartment where it reacts with the corresponding metal hydroxide that is formed at the titanium cathode. Note: The corresponding metal hydroxide is formed when the metal ions migrate to the negatively charged titanium cathode, and give up their electrons forming free metal, which then spontaneously reacts with the water forming the corresponding metal hydroxide, which remains dissolved in the electrolyte, and then reacts with the chlorine. The cell temperature of the cathode side of the apparatus is usually kept around 85 to 90 Celsius. If potassium chloride is used, the potassium chlorate will crystallize out of the the electrolyte in the cathode compartment due to its lack of solubility. If sodium or lithium chloride is used, the perchlorates will be formed on prolonged electrolysis.