structure formation and production of ozone

in nature, ultraviolet rays from The Sun break down oxygen in the atmosphere and turn ozone molecules.

technologically, it is obtained by the breakdown of the oxygen in the air with the help of electrical energy or pure oxygen.

in plate type generators

in CD type generators

in UV type lamps

ozone gas is the only natural disinfectant for commercial use. After completing its mission, ozone is always transformed into oxygen, which is its raw material.

ozone gas is inversely proportional to temperature. It is a gas with a very high oxidation power and is one of the strongest disinfectants known. The high oxidation force plays a fully active role in the elimination of microorganisms from ozone.

ozone disinfection destroys the microbes by dissolving them as the microbes break down the cell membrane. Ozone gas provides disinfection in approximately 4-10 minutes of contact in aqueous use. About 0.1-0.5 mg/lt ozone kills almost all microorganisms.
ozone has 3100 times stronger disinfection effect than chlorine under the same conditions. The unstable structure of ozone gas, as a result of disinfection process, open to the atmosphere in 30 minutes, 8-12 hours in closed packaging, without leaving any residual residue allows the raw material to be transformed into oxygen.

in a 1979 report by the World Health Organization, disinfection with ozone was proposed. With ozone gas being classified as reliable gases ( GRAS ) in 1997, the use of ozone in food began to become widespread.
in the Turkish food Codex, HACCP ( hazard analysis at Critical Control Points ) has made studies for the production of safe food mandatory.

due to its very strong oxidizing and very effective disinfecting , it is used as a germ killer in treatment plants providing drinking water worldwide.

the high oxidation force causes ozone to play a fully active role in the destruction of bacteria.

in addition, ozone is obtained through the breakdown of oxygen in the air, because of its unstable nature, it always turns into oxygen, which is its raw material after completing the disinfection task.

the fact that ozone gas is the only disinfectant that does not leave any residue after disinfection makes its use especially in the food industry advantageous compared to other disinfectants.

for ozone to melt in water, the temperature must be low and the pressure applied must be high.

formation mechanism

ozone in the stratosphere layer in the atmosphere is formed on one side by the influence of ultraviolet radiation, while disappearing on the other. The air mass in the stratosphere layer is constantly severely affected by ultraviolet radiation from the sun. At this stage, almost all of the ultraviolet-B (UV-B) rays that pose a great danger to living things on the surface of the earth are absorbed by the ozone layer in the stratosphere.

this

O3 + h is formed in the form of the υ ——> O2 + O reaction. (λ = wavelength & lt; 243 nm) as a result of this reaction, the ozone molecule breaks down, releasing an oxygen molecule and an oxygen atom. Where h is the plank constant; υ is the frequency of UV-B rays.

the formation mechanism of the ozone molecule

the new free oxygen molecule formed as a result of the above reaction reacts with the oxygen atom in the ozone layer to form the ozone molecule (O3) again.

O2 + O + M ———> O3 + M

Here M is a third molecule that carries the energy released during the reaction

Destroying mechanism

an ozone molecule (O3) breaks down into O2 and O when exposed to ultraviolet radiation. During fragmentation, atomic and molecular oxygen gain kinetic energy, increasing heat and causing the atmospheric temperature to rise.

ozone production is achieved by ultraviolet radiation with a wavelength less than 240 Nm. The breakdown of ozone occurs when the long wavelength higher than 320 Nm and the short wavelength in the range of 400 to 700 nm are exposed to ultraviolet radiation. In creating the ozone production and fragmentation zone, longer-wavelength photons are more easily processed into the atmosphere. Even if an ozone molecule absorbs low-energy ultraviolet radiation, it can break down into an oxygen molecule and a free oxygen atom.

the main chemicals that destroy ozone are compounds containing hydrogen, nitrogen, chlorine and bromine. HOx, ClOx, NOx or BrOx as X, the general reaction that destroys ozone if one of its roots is taken

X + O3 ——-> XO + O2
XO + O ——-> X + O2
———————–
O + O3 ——-> O2 + O2

it can be shown as

.

here it should be noted that a single catalyst can destroy thousands of ozons. In particular, the co-catalytic effect of ClOx and Brox plays a fundamental role in the destruction of ozone in the lower stratosphere.

Br

O + ClO ——-> Br + Cl + O2
Br + O3 ——-> BrO + O2
Cl + O3 ——-> ClO + O2
———————–
2O3 ————–> 3O2

the mechanism of the chlorine (Cl) atom to break down and destroy the ozone molecule

major chemical compounds that destroy ozone and their properties

the main chemical compounds that destroy ozone are chlorofluorocarbones (CFC2), carbon tetrachloride, methyl chloroform, methane and nitrous oxide, which are widely used in industry (Table 2). Their uses, their share in the total and their lifetimes in the atmosphere are given in the following chart.

table:Major chemical compounds that destroy ozone.
Name	Formula	use	percent (%) share of	Life (Years)
Halon-1301	CBrF3	fire extinguishers	4	110
methyl chloroform	CH3CCl33	Solvents	5	8
Carbon tetraklorur	CCl4	Solventler	8	67
CFC-113	C2Cl3F3	Solventler	12	90
CFC-11	CCl3F	Aerosoller, Foams, Refrigerants	26	74
CFC-12	CCl2F2	aerosols, foams, Refrigerants, Air conditioners	45	111

the thinning of the ozone layer means that more UV radiation reaches the surface of the Earth. Therefore, ozone protects the biosphere by absorbing most of the UV-B radiation and plays a vital role in the environment in which we live.

all theoretical and experimental studies show that the release of CFCs and halons into the atmosphere causes the ozone layer to disappear more and the Antarctic ozone hole to appear more clearly, especially in the spring period.