CN111905547A - Method for oxidizing low-concentration NO in gas by using hydrogen peroxide - Google Patents

Method for oxidizing low-concentration NO in gas by using hydrogen peroxide Download PDF

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CN111905547A
CN111905547A CN201910373743.6A CN201910373743A CN111905547A CN 111905547 A CN111905547 A CN 111905547A CN 201910373743 A CN201910373743 A CN 201910373743A CN 111905547 A CN111905547 A CN 111905547A
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hydrogen peroxide
concentration
gas
decomposition catalyst
low
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刘明
张菡英
刘森
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Shandong Normal University
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Shandong Normal University
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    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01D—SEPARATION
    • B01D53/00—Separation of gases or vapours; Recovering vapours of volatile solvents from gases; Chemical or biological purification of waste gases, e.g. engine exhaust gases, smoke, fumes, flue gases, aerosols
    • B01D53/34—Chemical or biological purification of waste gases
    • B01D53/74—General processes for purification of waste gases; Apparatus or devices specially adapted therefor
    • B01D53/77—Liquid phase processes
    • B01D53/78—Liquid phase processes with gas-liquid contact
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01D—SEPARATION
    • B01D53/00—Separation of gases or vapours; Recovering vapours of volatile solvents from gases; Chemical or biological purification of waste gases, e.g. engine exhaust gases, smoke, fumes, flue gases, aerosols
    • B01D53/34—Chemical or biological purification of waste gases
    • B01D53/46—Removing components of defined structure
    • B01D53/54—Nitrogen compounds
    • B01D53/56—Nitrogen oxides

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  • Chemical & Material Sciences (AREA)
  • Environmental & Geological Engineering (AREA)
  • Health & Medical Sciences (AREA)
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  • Analytical Chemistry (AREA)
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Abstract

The invention discloses a method for oxidizing low-concentration NO in gas by using hydrogen peroxide. The invention overcomes the technical prejudice that active oxygen is used for replacing H2O2The low-concentration NO in the gas is oxidized by the OH free radicals, so that the cost can be saved, and the method has a wide application prospect.

Description

Method for oxidizing low-concentration NO in gas by using hydrogen peroxide
Technical Field
The invention relates to a method for oxidizing low-concentration NO in gas, in particular to a method for oxidizing low-concentration NO in gas by using hydrogen peroxide.
Technical Field
NO is a low-valent oxide that is both oxidizing and reducing in nature. NO is a gas, the content of which in the atmosphere is originally a trace amount, but recently, along with the large-scale development of industrialization, a large amount of NO in industrial flue gas is discharged to the atmosphere along with the flue gas, so that the content of NO in the atmosphere is gradually increased. The presence of excessive NO, and the compounds produced by its presence, can cause significant environmental hazards, such as acid rain, haze contamination, and the like. Therefore, it is necessary to control the emission thereof. However, because NO in the exhaust gas has the characteristics of difficult adsorption, low concentration, low pressure and the like, the control of NO has not been implemented by a mature, wide-application and low-cost process so far. In the prior art, the method for controlling the emission mainly adopts an SCR (selective catalytic reduction) method, namely, reducing the nitrogen into elemental nitrogen by using a reducing agent under certain conditions. The method has the disadvantages of high operation cost, secondary pollution caused by reducing agents and the like.
The method for removing NO from the waste gas by using hydrogen peroxide is a trend of removing NO in the future.
In the prior art, for example, chinese patent CN103209755, there is a process for oxidizing NO with hydrogen peroxide, which is based on the idea that hydrogen peroxide is vaporized or atomized to generate highly oxidative OH radicals at a higher temperature (over 100 ℃), so that NO is oxidized by the OH radicals to become easily absorbable nitrogen oxides in a high valence state. The prior art can solve the problem of secondary pollution caused by an SCR reduction method, and can also produce byproducts such as nitrate, nitrous acid and the like. However, the temperature of many flue gases in the industry does not exceed 150 ℃, so that the flue gases need to be heated or the hydrogen peroxide needs to be heated, so that the cost is increased, the process is complicated, and the application occasions are limited.
Disclosure of Invention
Aiming at the technical problems, the invention provides a new idea and technical scheme different from the prior art, namely, an aqueous solution (hydrogen peroxide) of hydrogen peroxide is used for oxidizing low-concentration NO in gas to convert the low-concentration NO into high-valence nitrogen oxide which is easy to absorb, so that the aim of removing nitrogen-containing substances in flue gas is fulfilled.
The technical scheme of the invention is as follows:
a method for oxidizing low-concentration NO in gas by using hydrogen peroxide is characterized in that in a liquid state, the stability of the hydrogen peroxide is firstly destroyed to decompose the hydrogen peroxide to generate active oxygen, and then the gas containing low-concentration NO is contacted with the hydrogen peroxide to oxidize the low-concentration NO in the gas by the active oxygen.
Preferably, the active oxygen is generated by heating hydrogen peroxide to 50-95 deg.C.
Preferably, wherein the temperature is from 60 ℃ to 85 ℃.
Preferably, the active oxygen is generated by contacting hydrogen peroxide with a decomposition catalyst thereof.
Preferably, wherein the decomposition catalyst is a soluble base.
Preferably, wherein the decomposition catalyst is MnO2、CuO、FeO、Fe2O3、Al2O3、CeO2、Cr2O3One of, or a combination of, CoO.
Preferably, wherein the decomposition catalyst is Fe2+、Fe3+、Mn2+、Cu2+、Cr3+One or a combination of ions.
Preferably, the decomposition catalyst is one of copper powder, iron powder and aluminum powder or a combination thereof.
Preferably, the decomposition catalyst is one of brick grains, tile grains, cooked cement grains and volcanic stone grains or a combination thereof.
Preferably, the active oxygen is generated by heating hydrogen peroxide to a decomposition temperature of 50-95 deg.C and adding a decomposition catalyst to the hydrogen peroxide.
Through a plurality of experiments, the following results are found: although hydrogen peroxide has strong oxidizing property in a low-temperature environment (the temperature is lower than 50 ℃), hydrogen peroxide cannot oxidize NO in low-concentration NO even if the concentration of hydrogen peroxide reaches 30% or 40%. Moreover, the smaller the PH of hydrogen peroxide, the more stable the hydrogen peroxide is, but the greater the difficulty of oxidizing NO.
Experiments also show that if measures are taken, the concentration of NO in the gas can be obviously reduced and even can be changed to 0 if the hydrogen peroxide is decomposed and then is mixed with the gas containing low-concentration NO in a gas-liquid manner. At the same time, the pH in the liquid will gradually decrease. This indicates that NO, which is poorly soluble in water or lye, has been converted into higher nitrogen oxides, such as NO2、N2O3、N2O4Or N2O5And the like. The prior knowledge shows that higher oxides of nitrogen, such as NO2、N2O3、N2O4Or N2O5And the like, compared with NO, are easy to react with or dissolve in water and alkali liquor.
The knowledge shows that the electrode potential of the hydrogen peroxide is about 1.77V, and gradually decreases along with the increase of the PH value, and the electrode potential is about 0.88 under the alkaline condition.
According to experiments, under acidic and neutral conditions, the hydrogen peroxide cannot oxidize low-concentration NO in the gas, but under alkaline conditions, when the hydrogen peroxide is decomposed, the NO can be oxidized by the hydrogen peroxide.
When a soluble base is added to hydrogen peroxide, the soluble base releases OH-Ions, OH-Ions can destroy the stability of hydrogen peroxide in a short time to decompose the hydrogen peroxide, and at the moment, NO gas with low concentration is introduced, so that the concentration of NO in the gas can be obviously reduced, and sometimes even NO can be detected.
The soluble alkali is a substance that can be dissolved in water and can ionize hydroxide ions in water, such as sodium hydroxide, potassium hydroxide, calcium hydroxide, ammonia, alcohol amine, sodium carbonate, potassium carbonate, sodium bicarbonate, and potassium bicarbonate.
In addition, when the catalyst MnO is put into the hydrogen peroxide2Hydrogen peroxide also decomposes, and at this time hydrogen peroxide can also oxidize low concentration NO in the gas.
Through experiments, substances capable of causing decomposition of hydrogen peroxide are also: CuO, FeO, Fe2O3、Al2O3、CeO2、Cr2O3Metal oxides such as CoO; fe2+、Fe3+、Mn2+、Cu2+、Cr3+Plasma metal ions; if metal powder materials such as iron powder, aluminum powder, copper powder and the like are added into hydrogen peroxide, the hydrogen peroxide can be decomposed; the addition of impurity particles such as cooked cement particles, brick and tile particles, volcanic rock particles and the like into hydrogen peroxide can slightly cause the decomposition of hydrogen peroxide.
The aforementioned substances capable of causing decomposition of hydrogen peroxide, and other substances capable of causing decomposition of hydrogen peroxide, which are not listed in detail, are collectively referred to herein as decomposition catalysts for hydrogen peroxide.
In addition to the catalyst, another measure that can cause decomposition of hydrogen peroxide is heating the hydrogen peroxide. If 30% of hydrogen peroxide is heated, the temperature is lower than 40 ℃, the hydrogen peroxide is hardly decomposed, bubbles are generated in the hydrogen peroxide when the temperature reaches 50 ℃, and at the moment, gas containing NO is introduced, so that the NO content in the gas is reduced; the higher the temperature, the faster the hydrogen peroxide decomposes and the less the NO concentration becomes after the gas is let out.
However, it should be noted that when the heating temperature of the hydrogen peroxide is too high, the oxygen is emitted from the hydrogen peroxide2The more the portion O2NO is not reoxidized but becomes a loss. Therefore, the hydrogen peroxide is required to be decomposed and cannot be decomposed too quickly when being heated, and therefore, the heating temperature is preferably 60-85 ℃. However, when the temperature of the hydrogen peroxide reaches 95 ℃ or above, the water itself will boil, and it is difficult to ensure that the hydrogen peroxide can react with NO in a liquid state.
Relates to the generation of ineffective O by the decomposition of hydrogen peroxide2The same applies to the above-mentioned decomposition catalyst, and therefore the principle of the catalyst arrangement and design is to ensure that the hydrogen peroxide can be decomposed and to minimize the discharge of the oxygen-free gas.
In addition, ineffective O2The amount of the produced oxygen is also related to factors such as the concentration of the hydrogen peroxide, the amount and the form of the catalyst, the heating temperature of the hydrogen peroxide and the like, and the higher the concentration is, the more violent the decomposition is and the ineffective O is2The amount of (a) increases; the higher the temperature, the more violent the decomposition, the easier it is to oxidize NO, and the ineffective O2There is also an increase. If the catalyst is added while heating, the decomposition of the hydrogen peroxide is obviously accelerated, NO is easily oxidized, and the catalyst is ineffective2The amount of (a) also increases.
The prior knowledge and experiments can show that the NO with low concentration in the oxidizing gas is not hydrogen peroxide, but is generated during the decomposition of the NO.
It can be directly observed by naked eyes that bubbles are generated in the solution when the hydrogen peroxide is decomposed, and the bubble component is detected to be gas O2。
Because a large amount of O is generated when hydrogen peroxide is decomposed2At this time, O is present in the water2The concentration becomes extremely high, which makes the reaction:
2NO + O2= 2NO2
can be carried out in a positive direction, thereby oxidizing NO;
in addition, it is described in the literature that when hydrogen peroxide is decomposed by spectroscopic analysis, it can be estimated that free O appears. The electrode potential of O is 2.694, which is extremely high and can completely oxidize NO into higher nitrogen oxides.
O will react with O2Reaction to form O3，O3The electrode potential of (2) is 2.067, and NO can be oxidized.
Although the electrode potential is also high, the hydroxyl radicals are generated only under high temperature conditions, and the hydroxyl radicals are not generated even when the hydrogen peroxide is decomposed under low temperature conditions (less than 100 ℃ C.).
As described above, when hydrogen peroxide is decomposed, NO can be oxidized. The oxide can be gas O generated in liquid during decomposition of hydrogen peroxide2May be oxygen atom in a free state or O3。It is also possible that the three act together. Here, O generated when hydrogen peroxide is decomposed2O and O3Collectively referred to as active oxygen.
The oxidation of NO by hydrogen peroxide mainly depends on the action of active oxygen generated in liquid.
Has the advantages that:
1. the invention overcomes the technical prejudice that the active oxygen is generated instead of H2O2Either by itself or OH radicals to oxidize NO.
2. The invention applies the clean oxidant hydrogen peroxide to remove NO in the gas, thereby saving the cost, and being environment-friendly and sanitary.
Drawings
FIG. 1 is a flow chart of an apparatus of example 1;
FIG. 2 is a flowchart of the apparatus of example 6.
Detailed Description
Example 1
The technical scheme of the invention is explained in detail by combining the attached drawing 1:
1 is a nitrogen cylinder, 2 is an NO cylinder, 3 is a gas mixing chamber, 4 is an oxidation tank, 30% hydrogen peroxide is filled in the tank, the middle lower part of the tank is provided with a shower head 5, the gas aperture of the shower head is 1mm, 6 is a catalyst tank, and NaOH solution is filled in the tank. The connection relationship of the components is shown in figure 1.
Initially, valve 3 is closed and valve 4 is open. And opening the valve 1 and the valve 2, mixing the nitrogen and the NO in the gas mixing chamber 3, and measuring the concentration of the NO at the gas outlet 1 by a flue gas measuring instrument. The valves 1 and 2 were adjusted so that the measured NO concentration was 100mg/m3--1000mg/m3Internal value, e.g. 300mg/m3。
The valve 3 is opened while the valve 4 is closed, and the mixture gas enters the oxidation pond 5 from the shower head 5 and flows out from the gas outlet 2. The NO concentration is measured by a flue gas measuring instrument at the gas outlet 2, and the NO concentration is unchanged.
Valve 4 is opened while valve 3 is closed.
The valve 5 is then opened and the NaOH solution is injected into the oxidation basin 4, with bubbles appearing in the hydrogen peroxide shortly after the injection of the NaOH solution. The valve 3 is opened again and the valve 4 is closed, so that the mixed gas enters the oxidation pond 4 from the shower head 5 and flows out from the gas outlet 2. The NO concentration was measured at the outlet 2 with a flue gas measuring instrument. Through measurement, when the PH value of the hydrogen peroxide reaches 8, the NO concentration begins to decrease, and when the PH value reaches 14, the NO concentration measured by the flue gas measuring instrument is 0.
Example 2
Other conditions and procedures were the same as in example 1 except that the NaOH solution in the catalyst tank 6 was replaced with MnO2And (3) pulverizing. Measured when MnO2After the powder is added into the hydrogen peroxide, bubbles are blown out of the hydrogen peroxide, and the concentration of NO measured at the gas outlet 2 is reduced.
Example 3
Other conditions and procedures were the same as in example 1, and the NaOH solution in the catalyst tank 6 was replaced with iron powder. Through measurement, when the iron powder is added with hydrogen peroxide and a certain amount of hydrochloric acid is added into the hydrogen peroxide, bubbles are emitted from the hydrogen peroxide, and the concentration of NO measured at the gas outlet 2 is reduced.
Example 4
Other conditions and procedures were the same as in example 1 except that the NaOH solution in the catalyst tank 6 was replaced with FeCl3And (3) solution. Measured when FeCl is added3After the solution is added into the hydrogen peroxide, bubbles are blown out of the hydrogen peroxide, and the concentration of NO measured at the gas outlet 2 is reduced.
Example 5
Other conditions and procedures were the same as in example 1, and the NaOH solution in the catalyst tank 6 was replaced with fine boiled cement pellets. Through measurement, after the fine and cooked cement particles are added with hydrogen peroxide, bubbles of the hydrogen peroxide are blown out, and the concentration of NO measured at the gas outlet 2 is also reduced.
Example 6
The technical scheme of the invention is explained in detail with reference to the attached figure 2:
1 is a nitrogen cylinder, 2 is an NO cylinder, 3 is a gas mixing chamber, 4 is an oxidation tank, 30% hydrogen peroxide is filled in the tank, the middle lower part of the tank is provided with a shower nozzle 5, the gas aperture of the shower nozzle is 1mm, and 6 is a water bath. The connection relationship of the components is shown in figure 2.
Initially, valve 3 is closed and valve 4 is open. And opening the valve 1 and the valve 2, mixing the nitrogen and the NO in the gas mixing chamber 3, and measuring the concentration of the NO at the gas outlet 1 by a flue gas measuring instrument. The valves 1 and 2 were adjusted so that the measured NO concentration was 100mg/m3--1000mg/m3Internal value, e.g. 200mg/m3。
The water bath 6 is heated to 80 ℃, and then the oxidation pond 4 is placed. After a certain time, bubbles begin to emerge from the hydrogen peroxide in the oxidation pond 4. The valve 3 is opened while the valve 4 is closed, and the mixture gas enters the oxidation pond 4 from the shower head 5 and flows out from the gas outlet 2. The NO concentration was measured at the outlet 2 with a flue gas measuring instrument. It was measured that the concentration of NO becomes small at the gas outlet 2.

Claims (10)

1. A method for oxidizing low-concentration NO in gas by using hydrogen peroxide is characterized in that the stability of hydrogen peroxide is firstly destroyed to decompose the hydrogen peroxide to generate active oxygen, and then the gas containing low-concentration NO is contacted with the hydrogen peroxide to oxidize the low-concentration NO in the gas by the active oxygen.
2. The method of utilizing low concentration NO in hydrogen peroxide oxidizing gas as claimed in claim 1, wherein the active oxygen is generated by heating hydrogen peroxide to a temperature of 50-95 ℃.
3. The method for utilizing low concentration NO in hydrogen peroxide oxidizing gas according to claim 2, wherein the decomposition temperature is 60 ℃ to 85 ℃.
4. The method of utilizing low concentration NO in a hydrogen peroxide oxidizing gas as claimed in claim 1, wherein the active oxygen is generated by contacting hydrogen peroxide with a decomposition catalyst thereof.
5. The method for utilizing low concentration NO in hydrogen peroxide oxidation gas as claimed in claim 4, wherein the decomposition catalyst is soluble alkali.
6. The method of utilizing low concentration NO in hydrogen peroxide oxidizing gas as set forth in claim 4, wherein the decomposition catalyst is MnO2、CuO、FeO、Fe2O3、Al2O3、CeO2、Cr2O3One of, or a combination of, CoO.
7. The method for utilizing low concentration NO in hydrogen peroxide oxidizing gas as claimed in claim 3, wherein the decomposition catalyst is Fe2+、Fe3+、Mn2+、Cu2+、Cr3+One or a combination of ions.
8. The method for utilizing low-concentration NO in hydrogen peroxide oxidizing gas according to claim 4, wherein the decomposition catalyst is one or a combination of copper powder, iron powder and aluminum powder.
9. The method for utilizing low-concentration NO in hydrogen peroxide oxidation gas according to claim 4, wherein the decomposition catalyst is one or a combination of brick grains, tile grains, calcined cement grains and volcanic rock grains.
10. The method of claim 1, wherein the active oxygen is generated by heating the hydrogen peroxide to a temperature of 50-95 ℃ and adding a decomposition catalyst to the hydrogen peroxide.
CN201910373743.6A 2019-05-07 2019-05-07 Method for oxidizing low-concentration NO in gas by using hydrogen peroxide Pending CN111905547A (en)

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Citations (7)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US20050255022A1 (en) * 2004-05-11 2005-11-17 The Usa As Represented By The Administrator Of The National Aeronautics & Space Administration Emission control system
CN103007753A (en) * 2012-12-31 2013-04-03 上海电气石川岛电站环保工程有限公司 Heterogeneous Fenton reagent and preparation method and application thereof
CN103463978A (en) * 2013-09-30 2013-12-25 南京理工大学 Device and method for smoke simultaneous desulfurization and denitrification based on hydrogen peroxide catalytic oxidation
CN104941431A (en) * 2015-06-05 2015-09-30 北京中晶佳镁环境科技股份有限公司 Desulphurization and denitration device and method
CN106853328A (en) * 2016-03-11 2017-06-16 济南大学 A kind of hydrogen peroxide Efficient utilization method and device for low-temperature flue gas desulphurization denitration
CN107051168A (en) * 2017-06-14 2017-08-18 中冶京诚工程技术有限公司 Integrated device and method for low-temperature denitration of flue gas
CN107175118A (en) * 2017-05-09 2017-09-19 华北电力大学 The preparation method of iron-based heteropoly compound and the application that NO is removed in heterogeneous Fenton-like system

Patent Citations (7)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US20050255022A1 (en) * 2004-05-11 2005-11-17 The Usa As Represented By The Administrator Of The National Aeronautics & Space Administration Emission control system
CN103007753A (en) * 2012-12-31 2013-04-03 上海电气石川岛电站环保工程有限公司 Heterogeneous Fenton reagent and preparation method and application thereof
CN103463978A (en) * 2013-09-30 2013-12-25 南京理工大学 Device and method for smoke simultaneous desulfurization and denitrification based on hydrogen peroxide catalytic oxidation
CN104941431A (en) * 2015-06-05 2015-09-30 北京中晶佳镁环境科技股份有限公司 Desulphurization and denitration device and method
CN106853328A (en) * 2016-03-11 2017-06-16 济南大学 A kind of hydrogen peroxide Efficient utilization method and device for low-temperature flue gas desulphurization denitration
CN107175118A (en) * 2017-05-09 2017-09-19 华北电力大学 The preparation method of iron-based heteropoly compound and the application that NO is removed in heterogeneous Fenton-like system
CN107051168A (en) * 2017-06-14 2017-08-18 中冶京诚工程技术有限公司 Integrated device and method for low-temperature denitration of flue gas

Non-Patent Citations (2)

* Cited by examiner, † Cited by third party
Title
施悦等主编: "《环境氧化还原处理技术原理与应用》", 31 August 2013, 哈尔滨工业大学出版社 *
闫振甲等编著: "《高性能泡沫混凝土保温制品实用技术》", 30 June 2015, 中国建材工业出版社 *

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Application publication date: 20201110