What are the reaction conditions of nitrogen with oxygen?

In case of discharge.

Conditions: Under discharge conditions, nitrogen can be combined with oxygen to form nitric oxide.

Formula: N2 + O2 = Discharge = 2NO.

Nitric oxide rapidly combines with oxygen to produce nitrogen dioxide 2NO+O2=2NO2.

Nitrogen dioxide dissolves in water to form nitric acid, nitric oxide 3NO2 + H2O = 2HNO3 + NO.

Nitrogen, with the chemical formula N2, is usually a colorless and odorless gas, and nitrogen is generally less dense than air. Nitrogen is one of the main components of air. At standard atmospheric pressure, nitrogen becomes a colorless liquid when cooled to a point and liquid nitrogen becomes a snow-like solid when cooled to a point where it is cooled.

Nitrogen is chemically inactive, and it is difficult to react with other substances at room temperature, so it is often used to make preservatives. However, under high temperature and high energy conditions, it can undergo chemical changes with certain substances and be used to make new substances useful to human beings.

Generated in the case of discharge; Colorless nitric oxide. Nitric oxide is produced during thunder. However, nitric oxide is immediately oxidized by oxygen in the air to form brownish-yellow nitrogen dioxide, which is combined with water to form Hno3.

In case of alkali or some salt, nitrate is finally formed and fixed.

Under discharge conditions, nitrogen can be combined with oxygen to form nitric oxide.

n + o = discharge = 2no

Nitric oxide rapidly combines with oxygen to form nitrogen dioxide.

2no+o₂=2no₂

Nitrogen dioxide dissolves in water to form nitric acid.

Nitric Oxide: 3NO+HO=2HNO+NOoNitrogen is soluble in water and alcohol, but basically insoluble in most other liquids. It is essential in life, its compounds can be used as food or fertilizer, and nitrogen is used to make ammonia and nitric acid.

Nitrogen is basically an inert gas at ambient and moderate temperatures.

As a result, most metals are easy to handle with it. At elevated temperatures, nitrogen can be aggressive to metals and alloys.

There is no direct reaction between nitrogen and oxygen. At room temperature and pressure, nitrogen and oxygen are stable, and they do not undergo chemical reactions spontaneously.

However, nitrogen and oxygen can react in the presence of high temperatures, pressures, or appropriate catalysts. This reaction is called nitrogen oxidation reaction, also known as nitrogen oxidation reaction.

In a nitrogen oxidation reaction, nitrogen (N) and oxygen (O) undergo an oxidation reaction to form nitrogen oxides. This reaction usually requires high temperature and pressure and the presence of a catalyst, which can be either a metal or a metal oxide.

Here's an example reaction equation:

n₂ +o₂ 2no

In this reaction, nitrogen and oxygen react to form nitric oxide (NO).

Nitrogen oxidation reaction has an important application in industry. For example, it is used in the preparation of nitric acid and nitrate, compounds that are widely used as feedstock for fertilizers, chemicals, and synthetic chemicals. In addition, the nitrogen oxidation reaction is also associated with air pollution, as it produces harmful gases such as nitric oxide and nitrogen dioxide, which have potential effects on the atmospheric environment and human health.

The reaction that occurs between nitrogen and oxygen is the oxidation reaction of nitrogen with oxygen, which is commonly known as the nitrogen oxidation reaction. This reaction can produce a range of nitrogen oxides.

The most common nitrogen oxide is nitrogen dioxide (NO2). The chemical equation for this reaction is given below

2no + o2 ->2no2

In this reaction, two nitrogen (NO) molecules react with one oxygen (O2) molecule to produce two nitrogen dioxide (NO2) molecules.

This reaction usually occurs at high temperatures and pressures, such as in the combustion chamber of an internal combustion engine or in a high-temperature furnace in an industrial process.

It is important to note that nitrogen oxides in the atmosphere can have a negative impact on the environment and human health, so controlling and reducing nitrogen oxide emissions is very important to protect the environment and air quality.

Nitrogen and oxygen react chemically when discharged to form nitric oxide. The chemical equation is: N2 + O2 = Discharge = 2NO.

In addition, nitric oxide is then oxidized to nitrogen dioxide by oxygen in the air. Nitrogen dioxide reacts with water to form nitric acid, which eventually falls into the ground and reacts with minerals to form nitrate! i.e. nitrogenous fertilizers.

In daily life, we can also prepare high-purity oxygen and nitrogen by separating nitrogen and oxygen in the air at high or low temperatures.

Nitrogen and oxygen in the air react chemically when discharged to produce nitric oxide.

n2+o2=2no

The condition is discharge).

Under discharge conditions, nitrogen can be combined with oxygen to form nitric oxide.

These two gases can be combined in the event of an electric discharge, and this reaction can be used to prepare nitric acid.

Under natural conditions, when thunder, nitrogen and oxygen in the air will be combined in small amounts to form some nitrogen oxides, which will fall into the soil through the action of rain, this process is called natural nitrogen fixation, and its role is to apply natural nitrogen fertilizer to plants.

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This reaction is reversible and can occur at high temperatures, and the NO in the exhaust of the car is produced at high temperatures.

1. The reaction conditions of nitrogen and oxygen are extremely harsh, and there will be no backshot and tease at room temperature, and a large amount of energy needs to be provided by discharge (natural) or high temperature (artificial) to react.

2. If the two react exothermic, then the heat released can provide the activation energy of the reaction to the surrounding molecules, resulting in the reaction continuing under the condition that no energy is supplied to the outside world.

3. The air contains a large amount of nitrogen and oxygen, and if the reaction is exothermic, then the whole air will be burned up due to the reaction of nitrogen and oxygen. In fact, this has never happened. Therefore, the reaction must be endothermic. Raid sale.

1. Nitrogen and oxygen in the air will be chemically reversed in the case of discharge, which should generate nitric oxide N2+O2=2NO (the condition is discharge), and it is the only direct product of the reaction, although the nitrogen oxides are very filial. Other oxides of nitrogen are obtained by other means.

2. Because nitrogen and oxygen in the air will react chemically in the case of discharge to produce nitric oxide. Nitric oxide is then oxidized by oxygen in the air to nitrogen dioxide. Nitrogen dioxide reacts with water to form nitric acid, and nitric acid eventually reacts with minerals in the land to form nitrate!

i.e. nitrogenous fertilizers.

3. The nitrogen oxides in automobile exhaust are also the first to react n2+o2=2no between nitrogen and oxygen in the case of spark plug discharge, and then react with oxygen to convert into other forms of air pollutants.

The conditions under which nitric oxide reacts with oxygen are at room temperature and pressure.

The reaction between nitric oxide and oxygen is not reversible, and the reaction product is nitrogen dioxide. The relative molecular weight of nitric oxide is a colorless, odorless, and insoluble toxic gas in water. Since nitric oxide carries fibrous radicals, it is chemically reactive and can react without other conditions.

N2+O2 = (discharge) 2NO, 2NO+O2=2NO2, 3NO2+H2O=2HNO3+ NO.

The process of converting molecular nitrogen into ammonia by nitrogen-fixing organisms (such as various nitrogen-fixing bacteria) nitrogenase in nature.

Biological nitrogen fixation refers to the process by which nitrogen-fixing microorganisms reduce atmospheric nitrogen to ammonia.

The content of nitrogen fixed by nitrogen-fixing microorganisms is far from being compared with artificial nitrogen fixation and high-energy nitrogen fixation, and it can be said that nitrogen fixation in nature is mainly dependent on biological nitrogen fixation. Biological nitrogen fixation plays an important role in the nitrogen cycle in nature.

The rhizobia of leguminous plants, as well as the nitrogen-fixing spirobacteria in the roots of pastures and other grasses, and some prokaryotic lower plants, nitrogen-fixing cyanobacteria, and autogenous nitrogen-fixing bacteria, all contain nitrogenases, which have nitrogen-fixing effects. This category is biological nitrogen fixation that is naturally nitrogen-fixing.