What are the chemical properties of ozone? What is the chemical nature of ozone?

The chemical properties of ozone are extremely unstable, and it will slowly decompose into oxygen in both air and water, and its reaction formula is:

2o33o2285kj

Because a large amount of heat is released during decomposition, it is important to decompose when its content is in.

Above, it's easy**. However, the amount of ozone in ozonated air is difficult to exceed.

10. In the long history of ozone used in drinking water treatment, there has not been a single case of oxygen**. The content is:

The following ozone has a half-life of decomposition in air at room temperature and pressure.

Around 16h. As the temperature increases, the decomposition rate accelerates, and the temperature exceeds.

, the decomposition is very violent, reached.

At high temperatures, it is immediately converted to oxygen. Ozone breaks down much faster in water than in air. In an aqueous solution containing impurities, ozone quickly reverts to the oxygen that formed it. For example, the ozone concentration in water is.

mol/l(3mg/l)

, its half-life is.

30min but the decomposition rate is slower in pure water, such as in distilled water or tap water, the half-life is about.

20min20, however in secondary distilled water, elapses.

After 85 min, ozone decomposition only.

10. If the water temperature is close.

, ozone will become more stable.

The oxidizing capacity of ozone.

Ozone has a very strong oxidizing capacity, and its redox potential is second only to. f

This feature is mainly used in its applications. From the table.

. From the table.

It can be seen that the standard electrode potential of ozone is higher than that of oxidants such as oxygen, chlorine, chlorine dioxide and potassium permanganate, in addition to being lower than that of fluorine. This shows that ozone has the strongest oxidizing capacity among commonly used oxidants. At the same time, the product of ozone reaction is oxygen, so ozone is an efficient oxidant without secondary pollution.

1.The reaction between ozone and sodium generally produces sodium peroxide and oxygen.

2o3 + 2na = na2o2 + 2o22.The reaction between ozone and sulfur is divided into normal temperature and ignition, and the products are different under different conditions.

S + 2O3 (slow oxidation at room temperature) = SO2 + 2O23S + 2O3 (ignition) = 3SO2

3.Ozone and acids (HCl, HNO3), ozone is extremely oxidizing and can oxidize Cl-, but in HNO3, there is no element that can donate electrons, so it does not react. And NaOH also does not react, O3 has no acid properties.

o3 + 2hcl = h2o + cl2 + o24.The reaction of ozone with hydrogen, this must be ignited, and the product is water.

O3 + 3H2 (ignition) = 3H2O

5.In addition to the fact that ozone can be prepared by 302 = discharge = 2o3, what other methods can be used.

O2 can be irradiated with ultraviolet light, and it can be generated as well.

3O2 (ultraviolet) = 2O3

6.The reaction of inactive metals with ozone, which requires a slight heat, or a high temperature.

For example: Cu + O3 (Heating) = Cuo + O2Hg + O3 (Heating) = Hgo + O2 and so on.

7.The reaction of ozone with halogens does not react with F2, and Cl2 needs to be discharged, and the reaction of Br2 and I2 requires the participation of water.

4O3 + Cl2 (discharge) = 2ClO2 + 4O2BR2 + O3 + H2O = 2HBRO + O2I2 + O3 + H2O = 2Hio + O2Hio + 2O3 = HiO3 + 2O2 In general, O3 is involved in redox reaction products are usually O2. When the condition is ignition, or when the reducing agent is excessive, the resulting O2 will be further reduced. Oh.

The most prominent chemical property of ozone is its strong oxidizing properties.

Ozone has strong oxidizing properties, is a stronger oxidant than oxygen, can undergo oxidation reactions at lower temperatures, such as oxidizing silver to silver peroxide, leading sulfide to lead sulfate, and potassium iodide reaction to form iodine.

It is used as a strong oxidizing agent, bleaching agent, fur deodorant, air purifier, disinfectant and disinfectant, and disinfection and deodorization of drinking water. Ozone can be used to replace many catalytic oxidations or high-temperature oxidations in chemical production, simplifying production processes and increasing productivity. Liquid ozone can also be used as an oxidizer for rocket fuel.

Ozone, which has strong oxidizing properties.

Physics: At room temperature and pressure, ozone is a light blue gas with a special odor, and its density is greater than that of oxygen. Liquid ozone is dark blue with a boiling point of degrees Celsius, while solid ozone is purple-black with a melting point of -251 degrees Celsius.

Chemical: Unstable, extremely oxidizing, can be used for bleaching and disinfection.

Ozone is blue in liquid form and purple in solid state. It is different from oxygen and has a distinctly disgusting odor. Ozone has strong reactivity, is easy to decompose, very unstable, and will gradually decompose into oxygen at room temperature, its properties are more active than oxygen, and the specific gravity is twice that of ordinary air.

Ozone is accelerated by light, heat, water, metals, metal oxides, and other catalysts to decompose into oxygen. It is insoluble in liquid oxygen, carbon tetrachloride, etc. It has strong oxidizing properties, and can oxidize silver to silver oxide and lead sulfide to lead sulfate at room temperature.

Ozone can decolorize many organic pigments, which is very destructive to rubber and fibers, and easily oxidizes organic unsaturated compounds. Ozone is extremely stable in ice and has a half-life of 2000 years. Ozone can be tested using potassium iodide.

Ozone can eliminate planktonic bacteria in the air in a short time, and can neutralize and decompose toxic gases and remove foul odors. Ozone can therefore be used to purify air, drinking water, sterilize, treat industrial waste and as a bleaching agent.

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Problem description: Which country's trademarks are black and black girls?

Analysis: Some substances emitted into the atmosphere by human activities enter the stratosphere and chemically react with the ozone there, resulting in ozone depletion, and the phenomenon of reducing ozone concentration is called ozone layer depletion or ozone layer depletion.

Ozone in the ozone layer is naturally formed in the atmosphere higher above the ground, and its formation mechanism is:

The oxygen in the upper atmosphere is turned into free oxygen atoms by ultraviolet radiation from sunlight, and some of the free oxygen atoms combine with oxygen to form ozone, and 90% of ozone in the atmosphere is formed in this way.

Ozone molecules are unstable molecules, and ultraviolet radiation from the sun can not only produce ozone, but also decompose ozone to produce oxygen molecules and free oxygen atoms, so the concentration of ozone in the atmosphere depends on the dynamic equilibrium between its generation and decomposition rate.

Anthropogenic ozone depleting substances are mainly chlorofluoroalkanes (CFCs), which are widely used in refrigerators and air conditioners, foaming, and electronic device cleaning, as well as bromofluoroalkanes (halons) used in special occasions to extinguish fires. These substances are called ozone-depleting substances, and in order to protect the ozone layer, the international community has included these substances in the phase-out or controlled use list, so they are also called "controlled substances".

Ozone-depleting substances are very stable in the troposphere of the atmosphere and can stay for a long time, taking CFC12 as an example, it has a life span of about 120 years in the troposphere, so this kind of substances can diffuse to all parts of the atmosphere, but after reaching the stratosphere, it will be decomposed by the sun's ultraviolet radiation, releasing very active free chlorine atoms or bromine atoms, participating in a series of chemical reactions that lead to ozone depletion: free chlorine atoms or bromine atoms react with ozone molecules to produce chlorine or bromine monoxide, taking one of the oxygen atoms of the ozone molecule and turning it into an oxygen molecule. Chlorine or bromine monoxide reacts with free oxygen atoms, releasing "snatched" oxygen atoms to form more oxygen molecules and free chlorine atoms or free bromine atoms, and new free chlorine atoms or bromine atoms re-react with other ozone molecules to form oxygen molecules and chlorine or bromine monoxide again, such a reaction cycle continues, each free chlorine atom or bromine can destroy about 100,000 ozone molecules, which is why chlorofluoroalkanes or bromofluoroalkanes destroy the ozone layer.

What are the chemical and physical properties of O3?

Chemical properties: Extremely oxidizing!

Physical properties: ozone is a light blue gas with a special odor; It is denser than air and more soluble than oxygen and water. Liquid ozone is pale blue with a boiling point of degrees Celsius, and solid ozone is purple-black with a melting point of -251 degrees Celsius.