Nitric acid
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Nitric acid is manufactured industrially using the Ostwald process. The process involves reacting ammonia and oxygen gas over a platinum or rhodium catalyst at high temperatures and pressures to produce nitric oxide. The nitric oxide further reacts with oxygen to form nitrogen dioxide, which then reacts with water to produce nitric acid and nitric oxide in a cycle. The nitric acid is separated through distillation. One major use of nitric acid is in producing ammonium nitrate for nitrogen-based fertilizers.
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Nitric acid
Nitric acid is manufactured through Ostwald's process, which involves the catalytic oxidation of ammonia by air over a platinum catalyst heated to 800°C, forming nitric oxide. The nitric oxide is cooled and oxidized to nitrogen dioxide, which is then absorbed in water in an absorption tower to produce nitric acid solution. The dilute nitric acid is further concentrated by distillation under reduced pressure to obtain approximately 98% nitric acid.
HNO3 MANUFACTURING WITH PROCESS FLOW DIAGRAM
Here are two ways expenses are minimized in the Ostwald process:
1. The heat generated by the exothermic reactions is utilized to maintain the high temperature needed for the ammonia oxidation reaction, reducing energy costs.
2. Platinum-rhodium alloy is used as the catalyst. Platinum is very expensive but using it in an alloy with less costly rhodium allows the use of less platinum, lowering material costs.
Nitric acid Industries
Lecture Slides by Prof. Imitaz Ali at Ghulam Ishaq Khan Institute for Engineering Sciences and Technology (GIKI).
Nitric acid Preparation & Uses
Raw materials, Flow sheet diagram unit operation and unit process of nitric acid and hcl
physical and chemical properties of nitric acid
Hno3 lecture
Nitric Acid Manufacturing by Engineer Ghulam Abbas (Chemical Engineering Lecturer University of Gujrat)
Industrial manufacturing of Nitric acid
Industrial manufacturing of Nitric acid
This document contain detailed step of Industrial manufacturing of Nitric acid.
Manufacturing nitric acid by ostwald process
Nitric acid is a colourless liquid most commonly manufactured by Ostwald process which converts ammonia to nitric acid, nitric acid used for fertilizers, dye intermediates, explosives
Nitric acid
The document provides information about nitric acid, including its physical and chemical properties, manufacturing processes, uses, and production in Pakistan compared to worldwide. It describes nitric acid as a colorless liquid used to make fertilizers, dyes, and explosives. Three common industrial methods are discussed for manufacturing nitric acid: the Chile saltpeter method using sodium nitrate, Birkland-Eyde's method using air, and Ostwald's ammonia oxidation process. Nitric acid production in Pakistan is compared to global production levels, and major Pakistani nitric acid producers are listed.
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Nitric acid
Nitric acid is manufactured through Ostwald's process, which involves the catalytic oxidation of ammonia by air over a platinum catalyst heated to 800°C, forming nitric oxide. The nitric oxide is cooled and oxidized to nitrogen dioxide, which is then absorbed in water in an absorption tower to produce nitric acid solution. The dilute nitric acid is further concentrated by distillation under reduced pressure to obtain approximately 98% nitric acid.
HNO3 MANUFACTURING WITH PROCESS FLOW DIAGRAM
Here are two ways expenses are minimized in the Ostwald process:
1. The heat generated by the exothermic reactions is utilized to maintain the high temperature needed for the ammonia oxidation reaction, reducing energy costs.
2. Platinum-rhodium alloy is used as the catalyst. Platinum is very expensive but using it in an alloy with less costly rhodium allows the use of less platinum, lowering material costs.
Nitric acid Industries
Lecture Slides by Prof. Imitaz Ali at Ghulam Ishaq Khan Institute for Engineering Sciences and Technology (GIKI).
Nitric acid Preparation & Uses
Raw materials, Flow sheet diagram unit operation and unit process of nitric acid and hcl
physical and chemical properties of nitric acid
Hno3 lecture
Nitric Acid Manufacturing by Engineer Ghulam Abbas (Chemical Engineering Lecturer University of Gujrat)
Industrial manufacturing of Nitric acid
Industrial manufacturing of Nitric acid
This document contain detailed step of Industrial manufacturing of Nitric acid.
Manufacturing nitric acid by ostwald process
Nitric acid is a colourless liquid most commonly manufactured by Ostwald process which converts ammonia to nitric acid, nitric acid used for fertilizers, dye intermediates, explosives
Nitric acid
The document provides information about nitric acid, including its physical and chemical properties, manufacturing processes, uses, and production in Pakistan compared to worldwide. It describes nitric acid as a colorless liquid used to make fertilizers, dyes, and explosives. Three common industrial methods are discussed for manufacturing nitric acid: the Chile saltpeter method using sodium nitrate, Birkland-Eyde's method using air, and Ostwald's ammonia oxidation process. Nitric acid production in Pakistan is compared to global production levels, and major Pakistani nitric acid producers are listed.
Nitric acid preparation & uses
The document discusses the production and properties of nitric acid and hydrochloric acid. It describes the main industrial processes for manufacturing each acid, including the Ostwald process for nitric acid production and electrolysis of sodium chloride to produce chlorine for hydrochloric acid synthesis. Key safety considerations for acid storage are outlined, emphasizing the need for corrosion-resistant materials and segregation of different acid types.
Nitric acid by oxidation process
The document summarizes the nitric acid by oxidation process. The process involves:
a) Catalytic oxidation of ammonia with oxygen over platinum catalyst to produce nitrogen monoxide.
b) Oxidation of nitrogen monoxide to nitrogen dioxide which is then absorbed in water to produce nitric acid.
c) Concentration of the nitric acid product to 57-60% strength through a series of absorption towers.
Nitric acid Preparation & Uses
Nitric acid is a strong oxidizing agent that is colorless and highly corrosive. It is produced industrially via the Ostwald process, which involves the oxidation of ammonia to nitric oxide using a platinum catalyst and air, followed by the oxidation of nitric oxide to nitrogen dioxide and its absorption in water to form nitric acid. Nitric acid has a variety of uses including as a fertilizer component and nitrating agent for explosives. Hydrochloric acid is also a strong corrosive acid that is produced from chlorination byproducts or by reacting metallic chlorides with sulfuric acid. It is used in a variety of industrial processes.
Nitric acid
Nitric acid is produced through a two-step Ostwald process involving the oxidation of ammonia to nitric oxide followed by the absorption of nitrogen dioxide in water to form nitric acid. It is a colorless, corrosive, and toxic mineral acid that is commonly used in fertilizers and explosives due to its oxidizing properties. Some of the major producers of nitric acid in Pakistan include Ahmad Chemicals, Karakuram Scientific Company, and several fertilizer companies.
Nitric acid Preparation & Uses Raw materials, Flow sheet diagram unit operat...
Raw materials, Flow sheet diagram unit operation and unit process of nitric acid and hcl
Nitric acid Preparation & Uses
Ostwald's process
Nitric acid is produced through a multi-step industrial process involving the oxidation of ammonia. Ammonia is oxidized to nitric oxide at high temperatures in the presence of a platinum catalyst. The nitric oxide is then cooled and further oxidized to nitrogen dioxide, which is absorbed in water to form nitric acid. The dilute nitric acid is concentrated through reabsorption, resulting in a 68% concentrated solution used in fertilizer production, explosives, and other applications requiring a strong oxidizing acid.
Nitric acid Preparation & Uses
PHYSICAL CHEMICAL PROPERTIES
CHILE SALTPETRE METHOD (By NaNO3/KNO3)
BRIKLAND EYDE’S METHOD BY USING AIR
OSTWALD ’S METHOD BY AMMONIA SOLVEY PROCESS
Nitric acid
Nitric acid is a strong acid that is colorless as a pure liquid but commercial nitric acid may be yellowish-brown. It is produced through a three-stage process involving the oxidation of ammonia over a platinum catalyst. It has many industrial uses including in explosives, fertilizers, dyes, and others. When reacted with metals, it produces metal nitrates and oxides of nitrogen. It is both an oxidizing and acidifying agent that can cause explosions when reacted with some metals like sodium or potassium. The document provides details on the manufacture, properties, uses, and reactions of nitric acid.
Nitric acid Preparation & Uses Raw materials, Flow sheet diagram unit operat...
Nitric acid and hydrochloric acid are strong acids with various industrial uses. Nitric acid is produced through the Ostwald process involving ammonia oxidation over a platinum catalyst. It is used to make explosives, fertilizers, and other chemicals. Proper storage of nitric and hydrochloric acids is important due to their corrosive nature and potential for dangerous reactions. They should be kept in acid-resistant containers in a well-ventilated chemical storage area.
preparation and uses of nitric acid
Nitric acid is a colorless liquid that is strongly acidic and corrosive. It is produced industrially through the Ostwald process, which involves a three-step oxidation of ammonia using air over a platinum catalyst. Nitric acid is used to produce fertilizers, explosives like TNT, and other chemicals. It is also used in metal purification and to make aqua regia for dissolving noble metals. Proper precautions must be taken when handling nitric acid due to its corrosive nature and potential to cause burns or lung damage.
Nitric acid Preparation & Uses
Nitric acid and hydrochloric acid are strong acids that are highly soluble in water. Nitric acid is produced commercially via the Ostwald process, which involves catalytic oxidation of ammonia to produce nitric oxide, which is then oxidized to nitrogen dioxide and absorbed in water to form nitric acid. Hydrochloric acid is produced via electrolysis of sodium chloride to produce chlorine, which is then combined with hydrogen to form hydrochloric acid. Both acids are colorless liquids with pungent odors that are widely used in industry, such as in fertilizer production and cleaning applications. Proper storage of the acids requires acid resistant containers and secondary containment to mitigate hazards.
Nitric acid presentation
Nitric acid is a colorless, corrosive, and toxic mineral acid. It is composed of one hydrogen atom, one nitrogen atom, and three oxygen atoms. Nitric acid was first identified in the 9th century and has had various names over time. It was first synthesized in the early 20th century and was used by Germans prior to WWI to produce nitrates for weapons. Nitric acid is commonly used in industry, agriculture, and for making explosives and rocket fuel due to its strong oxidizing properties. It poses severe health and safety hazards if mishandled.
Nitric acid by arc process
Nitric acid is a strong, corrosive mineral acid that is colorless, though older samples appear yellowish. It is produced commercially at 68% concentration through three main methods, including the arc process. The arc process involves passing air through an electric arc chamber where nitrogen and oxygen combine at high temperatures to form nitric oxide, which is then oxidized to nitrogen dioxide and absorbed to produce nitric acid.
7.05 la chateliers principle
The Ostwald process is a 3-step reaction that oxidizes ammonia to produce nitric acid in a more economical way than directly reacting nitrogen with oxygen. Wilhelm Ostwald patented the process in 1902. It involves reacting ammonia with oxygen over a platinum catalyst to produce NO, then reacting the NO with oxygen to produce NO2, and finally reacting the NO2 with water to produce nitric acid. The process allows for cheap, mass production of nitric acid which is used to produce ammonium nitrate fertilizer and explosives like nitroglycerin and trinitrotoluene.
Manufacture of Nitric acid by chile saltpetre
The document describes the process for manufacturing nitric acid (HNO3) using Chile saltpeter. Chile saltpeter contains sodium nitrate (NaNO3), potassium nitrate, and sodium chloride. In the process, a mixture of Chile saltpeter and sulfuric acid is heated in a cast iron retort. The vapors produced are cooled and condensed to collect concentrated HNO3. Any uncondensed vapors are scrubbed with water to collect dilute HNO3. The key reaction is between sodium nitrate and sulfuric acid to produce sodium bisulfate and nitric acid.
Nitric acid Preparation & Uses
This document discusses nitric acid and hydrochloric acid (HCl). It describes the preparation and uses of nitric acid, including in fertilizers, plastics, dyes, and explosives. The disadvantages of nitric acid are that it is highly corrosive and can damage lungs if inhaled or the throat and stomach if swallowed. The document then introduces HCl as a clear, colorless, and corrosive acid found in gastric acid. Methods of producing HCl include burning elements, reactions of organic byproducts and metallic chlorides with sulfuric acid, waste incineration, and decomposition of hydrated heavy metals.
Nitric acid
This document discusses the usage of nitric acid, the pollution it causes, and ways to prevent that pollution. Nitric acid is used widely in industries like fertilizer production, food processing, and gold purification. It pollutes the air through nitrogen oxide emissions which cause acid rain, and water through discharge of waste products. Prevention efforts include installing pollution control devices, refining waste before discharge, using cleaner fuels, and increasing tree planting.
Ammonium Nitrate
The Home Ministry has asked for a ban on ammonium nitrate production in India due to safety risks. This would negatively impact ammonium nitrate producers. Stakeholders need to consider how important ammonium nitrate is for the country's economy and find ways to mitigate risks to producers. Ammonium nitrate is a key ingredient in explosives and is widely used in mining and infrastructure development, which are important industries for India's growth.
Nitrogen ttrichloride --- revised
The document discusses the risks and controls associated with nitrogen trichloride (NCl3) in chlorine production and storage facilities. NCl3 is a hazardous compound that can form and accumulate during chlorine production from brine. Even small amounts of NCl3 can detonate violently if not properly handled. The document outlines areas of potential risk, how NCl3 forms, its explosive hazards, methods to detect it, and ways to control and limit its formation to improve safety.
HCl manufacturing salt sulphuric acid process
This document discusses the production and manufacturing of hydrochloric acid (HCl). HCl exists as a solution of hydrogen chloride gas in water and can exist in solid, liquid, and gas states. It has been produced since the 15th century through various methods. Today, the most common method is absorbing the hydrogen chloride by-product from other chemical manufacturing processes, such as chlorinating hydrocarbons. HCl is manufactured through processes like reacting salt and sulfuric acid, synthesizing from hydrogen and chlorine gas, absorbing by-products, and more. When produced from salt and sulfuric acid, the reactants are heated in a furnace to produce HCl gas and sodium sulfate as a byproduct. The hot H
Presentation Nitric Acid
Nitric acid is a strong acid that is colorless as a pure liquid but commercial samples may appear yellowish. It is highly corrosive and a strong oxidizer. Nitric acid is produced industrially via the Ostwald process, which involves ammonia oxidation over a platinum catalyst in three steps: primary oxidation to nitric oxide, secondary oxidation to nitrogen dioxide, and absorption of nitrogen dioxide in water to form nitric acid. Nitric acid has many industrial and laboratory uses including fertilizer and explosive production.
DESIGN PROJECT 2013
This document provides a design for a plant to produce 400,000 metric tonnes of nitric acid per year using the Ostwald process. It selects a single pressure process as most advantageous after considering several factors such as efficient energy management. The process involves vaporizing ammonia at 1000 kPa and 35°C using process heat, then superheating it to 80°C with steam before mixing it with compressed air in a converter reactor over a platinum catalyst to produce nitrogen oxides, which are then absorbed in water to form the nitric acid product. The plant is estimated to cost ₦5.41 billion with a 26.25% return on investment and a 3 year, 7 month payback period, making the project technically
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Nitric acid preparation & uses
The document discusses the production and properties of nitric acid and hydrochloric acid. It describes the main industrial processes for manufacturing each acid, including the Ostwald process for nitric acid production and electrolysis of sodium chloride to produce chlorine for hydrochloric acid synthesis. Key safety considerations for acid storage are outlined, emphasizing the need for corrosion-resistant materials and segregation of different acid types.
Nitric acid by oxidation process
The document summarizes the nitric acid by oxidation process. The process involves:
a) Catalytic oxidation of ammonia with oxygen over platinum catalyst to produce nitrogen monoxide.
b) Oxidation of nitrogen monoxide to nitrogen dioxide which is then absorbed in water to produce nitric acid.
c) Concentration of the nitric acid product to 57-60% strength through a series of absorption towers.
Nitric acid Preparation & Uses
Nitric acid is a strong oxidizing agent that is colorless and highly corrosive. It is produced industrially via the Ostwald process, which involves the oxidation of ammonia to nitric oxide using a platinum catalyst and air, followed by the oxidation of nitric oxide to nitrogen dioxide and its absorption in water to form nitric acid. Nitric acid has a variety of uses including as a fertilizer component and nitrating agent for explosives. Hydrochloric acid is also a strong corrosive acid that is produced from chlorination byproducts or by reacting metallic chlorides with sulfuric acid. It is used in a variety of industrial processes.
Nitric acid
Nitric acid is produced through a two-step Ostwald process involving the oxidation of ammonia to nitric oxide followed by the absorption of nitrogen dioxide in water to form nitric acid. It is a colorless, corrosive, and toxic mineral acid that is commonly used in fertilizers and explosives due to its oxidizing properties. Some of the major producers of nitric acid in Pakistan include Ahmad Chemicals, Karakuram Scientific Company, and several fertilizer companies.
Nitric acid Preparation & Uses Raw materials, Flow sheet diagram unit operat...
Raw materials, Flow sheet diagram unit operation and unit process of nitric acid and hcl
Nitric acid Preparation & Uses
Ostwald's process
Nitric acid is produced through a multi-step industrial process involving the oxidation of ammonia. Ammonia is oxidized to nitric oxide at high temperatures in the presence of a platinum catalyst. The nitric oxide is then cooled and further oxidized to nitrogen dioxide, which is absorbed in water to form nitric acid. The dilute nitric acid is concentrated through reabsorption, resulting in a 68% concentrated solution used in fertilizer production, explosives, and other applications requiring a strong oxidizing acid.
Nitric acid Preparation & Uses
PHYSICAL CHEMICAL PROPERTIES
CHILE SALTPETRE METHOD (By NaNO3/KNO3)
BRIKLAND EYDE’S METHOD BY USING AIR
OSTWALD ’S METHOD BY AMMONIA SOLVEY PROCESS
Nitric acid
Nitric acid is a strong acid that is colorless as a pure liquid but commercial nitric acid may be yellowish-brown. It is produced through a three-stage process involving the oxidation of ammonia over a platinum catalyst. It has many industrial uses including in explosives, fertilizers, dyes, and others. When reacted with metals, it produces metal nitrates and oxides of nitrogen. It is both an oxidizing and acidifying agent that can cause explosions when reacted with some metals like sodium or potassium. The document provides details on the manufacture, properties, uses, and reactions of nitric acid.
Nitric acid Preparation & Uses Raw materials, Flow sheet diagram unit operat...
Nitric acid and hydrochloric acid are strong acids with various industrial uses. Nitric acid is produced through the Ostwald process involving ammonia oxidation over a platinum catalyst. It is used to make explosives, fertilizers, and other chemicals. Proper storage of nitric and hydrochloric acids is important due to their corrosive nature and potential for dangerous reactions. They should be kept in acid-resistant containers in a well-ventilated chemical storage area.
preparation and uses of nitric acid
Nitric acid is a colorless liquid that is strongly acidic and corrosive. It is produced industrially through the Ostwald process, which involves a three-step oxidation of ammonia using air over a platinum catalyst. Nitric acid is used to produce fertilizers, explosives like TNT, and other chemicals. It is also used in metal purification and to make aqua regia for dissolving noble metals. Proper precautions must be taken when handling nitric acid due to its corrosive nature and potential to cause burns or lung damage.
Nitric acid Preparation & Uses
Nitric acid and hydrochloric acid are strong acids that are highly soluble in water. Nitric acid is produced commercially via the Ostwald process, which involves catalytic oxidation of ammonia to produce nitric oxide, which is then oxidized to nitrogen dioxide and absorbed in water to form nitric acid. Hydrochloric acid is produced via electrolysis of sodium chloride to produce chlorine, which is then combined with hydrogen to form hydrochloric acid. Both acids are colorless liquids with pungent odors that are widely used in industry, such as in fertilizer production and cleaning applications. Proper storage of the acids requires acid resistant containers and secondary containment to mitigate hazards.
Nitric acid presentation
Nitric acid is a colorless, corrosive, and toxic mineral acid. It is composed of one hydrogen atom, one nitrogen atom, and three oxygen atoms. Nitric acid was first identified in the 9th century and has had various names over time. It was first synthesized in the early 20th century and was used by Germans prior to WWI to produce nitrates for weapons. Nitric acid is commonly used in industry, agriculture, and for making explosives and rocket fuel due to its strong oxidizing properties. It poses severe health and safety hazards if mishandled.
Nitric acid by arc process
Nitric acid is a strong, corrosive mineral acid that is colorless, though older samples appear yellowish. It is produced commercially at 68% concentration through three main methods, including the arc process. The arc process involves passing air through an electric arc chamber where nitrogen and oxygen combine at high temperatures to form nitric oxide, which is then oxidized to nitrogen dioxide and absorbed to produce nitric acid.
7.05 la chateliers principle
The Ostwald process is a 3-step reaction that oxidizes ammonia to produce nitric acid in a more economical way than directly reacting nitrogen with oxygen. Wilhelm Ostwald patented the process in 1902. It involves reacting ammonia with oxygen over a platinum catalyst to produce NO, then reacting the NO with oxygen to produce NO2, and finally reacting the NO2 with water to produce nitric acid. The process allows for cheap, mass production of nitric acid which is used to produce ammonium nitrate fertilizer and explosives like nitroglycerin and trinitrotoluene.
Manufacture of Nitric acid by chile saltpetre
The document describes the process for manufacturing nitric acid (HNO3) using Chile saltpeter. Chile saltpeter contains sodium nitrate (NaNO3), potassium nitrate, and sodium chloride. In the process, a mixture of Chile saltpeter and sulfuric acid is heated in a cast iron retort. The vapors produced are cooled and condensed to collect concentrated HNO3. Any uncondensed vapors are scrubbed with water to collect dilute HNO3. The key reaction is between sodium nitrate and sulfuric acid to produce sodium bisulfate and nitric acid.
Nitric acid Preparation & Uses
This document discusses nitric acid and hydrochloric acid (HCl). It describes the preparation and uses of nitric acid, including in fertilizers, plastics, dyes, and explosives. The disadvantages of nitric acid are that it is highly corrosive and can damage lungs if inhaled or the throat and stomach if swallowed. The document then introduces HCl as a clear, colorless, and corrosive acid found in gastric acid. Methods of producing HCl include burning elements, reactions of organic byproducts and metallic chlorides with sulfuric acid, waste incineration, and decomposition of hydrated heavy metals.
Nitric acid
This document discusses the usage of nitric acid, the pollution it causes, and ways to prevent that pollution. Nitric acid is used widely in industries like fertilizer production, food processing, and gold purification. It pollutes the air through nitrogen oxide emissions which cause acid rain, and water through discharge of waste products. Prevention efforts include installing pollution control devices, refining waste before discharge, using cleaner fuels, and increasing tree planting.
Ammonium Nitrate
The Home Ministry has asked for a ban on ammonium nitrate production in India due to safety risks. This would negatively impact ammonium nitrate producers. Stakeholders need to consider how important ammonium nitrate is for the country's economy and find ways to mitigate risks to producers. Ammonium nitrate is a key ingredient in explosives and is widely used in mining and infrastructure development, which are important industries for India's growth.
Nitrogen ttrichloride --- revised
The document discusses the risks and controls associated with nitrogen trichloride (NCl3) in chlorine production and storage facilities. NCl3 is a hazardous compound that can form and accumulate during chlorine production from brine. Even small amounts of NCl3 can detonate violently if not properly handled. The document outlines areas of potential risk, how NCl3 forms, its explosive hazards, methods to detect it, and ways to control and limit its formation to improve safety.
HCl manufacturing salt sulphuric acid process
This document discusses the production and manufacturing of hydrochloric acid (HCl). HCl exists as a solution of hydrogen chloride gas in water and can exist in solid, liquid, and gas states. It has been produced since the 15th century through various methods. Today, the most common method is absorbing the hydrogen chloride by-product from other chemical manufacturing processes, such as chlorinating hydrocarbons. HCl is manufactured through processes like reacting salt and sulfuric acid, synthesizing from hydrogen and chlorine gas, absorbing by-products, and more. When produced from salt and sulfuric acid, the reactants are heated in a furnace to produce HCl gas and sodium sulfate as a byproduct. The hot H
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Nitric acid Preparation & Uses Raw materials, Flow sheet diagram unit operat...
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Nitric acid Preparation & Uses Raw materials, Flow sheet diagram unit operat...
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Presentation Nitric Acid
Nitric acid is a strong acid that is colorless as a pure liquid but commercial samples may appear yellowish. It is highly corrosive and a strong oxidizer. Nitric acid is produced industrially via the Ostwald process, which involves ammonia oxidation over a platinum catalyst in three steps: primary oxidation to nitric oxide, secondary oxidation to nitrogen dioxide, and absorption of nitrogen dioxide in water to form nitric acid. Nitric acid has many industrial and laboratory uses including fertilizer and explosive production.
DESIGN PROJECT 2013
This document provides a design for a plant to produce 400,000 metric tonnes of nitric acid per year using the Ostwald process. It selects a single pressure process as most advantageous after considering several factors such as efficient energy management. The process involves vaporizing ammonia at 1000 kPa and 35°C using process heat, then superheating it to 80°C with steam before mixing it with compressed air in a converter reactor over a platinum catalyst to produce nitrogen oxides, which are then absorbed in water to form the nitric acid product. The plant is estimated to cost ₦5.41 billion with a 26.25% return on investment and a 3 year, 7 month payback period, making the project technically
Nitric acid
Nitric acid is a colorless liquid that is highly corrosive. It was first discovered in the 13th century and was known as aqua fortis. Nitric acid can be produced via the sodium nitrate process or by oxidizing ammonia. It is commonly used to make fertilizers and as a cleaning agent. While useful, nitric acid must be handled with care due to its corrosive nature.
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The production of nitric acid begins with natural gas or petroleum gas being converted into ammonia. Ammonia is then oxidized by reacting it with oxygen, forming nitrogen dioxide gas. This gas is absorbed by water, producing nitric acid. There are two main separation processes used: separation by barriers to remove sulfur from natural gas, and separation by solid agents to extract carbon dioxide when producing ammonia. Ammonia is then oxidized using air heated by a catalyst, forming nitrogen dioxide which is absorbed by water to create nitric acid.
Artificial Nitrogen Fixation
This document discusses nitrogen fixation, which is the process of converting atmospheric nitrogen gas into ammonia or other nitrogen compounds that can be used by plants and other organisms. It is difficult to fix nitrogen because nitrogen gas is very stable and its triple bonds are hard to break. The document outlines the Haber-Bosch process and Birkeland-Eyde process for industrial nitrogen fixation. Recent research aims to develop more efficient artificial and biological methods of nitrogen fixation, such as through transition metal complexes or engineering nitrogen fixation into food crops.
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This document summarizes the synthesis and characterization of a metal-organic framework (MOF) and subsequent postsynthetic modifications. Specifically, it details the synthesis of [Zn(bdc-NH2)2(dabco)] (DMOF-1-NH2, compound 1) and its activation. It then describes the covalent modification of compound 1 with diketene to introduce a ketoamide tag, forming compound 2. Finally, it explores dative modifications of compound 2 through treatment with KOtBu, ZnEt2, and [Rh2(μ-Cl)2(CO)4], forming compounds 3, 4, and 5 respectively, as evidenced by analytical techniques.
BigontheinsideMOFs
Metal-organic frameworks (MOFs) are highly porous materials consisting of metal atoms or clusters linked by organic molecules. MOFs have potential applications in hydrogen storage, methane storage, and carbon dioxide capture due to their ability to store gases at high densities through surface bonding. Australian researchers Matthew Hill and David Turner collaborate on using MOFs for gas storage and have achieved several world records. Their research utilizes synchrotron facilities to characterize MOF crystal structures, map their formation, and modify them for improved properties and applications.
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This study synthesized HKUST-1 metal organic framework nanoparticles using a sonochemical method for enhanced gas adsorption performance. Sonochemical synthesis produced HKUST-1 particles in the range of 30-60 nm with high surface area of 1797 m2/g. Testing showed the nanoparticles reduced CO2 concentration in a gas stream by 28.65% over 72 minutes. The nanoparticles were also incorporated into electrospun nanofibers to create MOF-loaded fiber membranes for gas adsorption applications.
Scintillating Metal Organic Frameworks
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Electro chemistry
Electrochemistry is a branch of chemistry that studies chemical reactions which take place in a solution at the interface of an electron conductor (a metal or a semiconductor) and an ionic conductor (the electrolyte), and which involve electron transfer between the electrode and the electrolyte or species in solution. It studies the exchange of chemical and electrical energy. The document provides an overview of electrochemistry prepared by three students from the University of Slemani's School of Science Chemistry Department.
Mof´s. By Nelson Giovanny Rincon Silva.
This document summarizes metal-organic frameworks (MOFs), including their properties and applications. MOFs are highly porous materials formed by combining metal ions or metal clusters with organic ligands. They have extremely large surface areas, often exceeding 7,000 m2/g. Due to their tunable porous structures, MOFs show promise for applications such as gas storage, carbon capture, catalysis, and luminescence. While MOF research has advanced significantly in recent decades, further developing their potential applications and improving stability remains an active area of research.
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This document summarizes research on the synthesis, characterization, and application of mesoporous niobium and tantalum oxides in heterogeneous catalysis. Mesoporous transition metal oxides were synthesized using a ligand-assisted templating approach with surfactants. Characterization techniques including powder XRD, nitrogen adsorption, SEM, TEM, FT-IR and NMR confirmed the mesoporous structure. The materials were tested in benzylation, alkylation and isomerization reactions and showed high activity and selectivity due to their high surface area and acidity. Pore size effects on catalytic performance were also investigated.
Ammonia
This document discusses ammonia, including its physical, chemical, and structural properties. It describes the Haber-Bosch process for producing ammonia through the reaction of nitrogen and hydrogen gases. Modern plants first convert natural gas to hydrogen, then combine it with nitrogen to make ammonia. The main industrial uses of ammonia are in fertilizer production and household cleaning. Secondary uses include refrigeration and as a lifting gas. In the laboratory, ammonia is used to make other nitrogen compounds and as a solvent. Exposure to high levels of ammonia can harm the environment and cause health issues in humans and animals such as increased blood pressure, mental effects, and damage to the esophagus from ingestion.
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Sulfuric Acid.pptx
Sulfuric acid is produced via the contact process, which involves three main steps:
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3) Sulfur trioxide is dissolved in concentrated sulfuric acid to form oleum, which is then diluted with water to produce 98% sulfuric acid.
Nitric acid preparation
Nitric acid is produced commercially using three main methods: the Chile saltpetre method using sodium nitrate, Birkeland-Eyde's method using air, and Ostwald's ammonia oxidation process. The Ostwald process, which involves oxidizing ammonia over a platinum catalyst at 800°C, is now the primary industrial method. Nitric acid is a strong oxidizing agent and corrosive liquid used to produce fertilizers, explosives, and other chemicals. Proper safety equipment like chemical gloves and goggles should be worn when handling it due to its ability to cause severe burns.
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Sodium hydroxide (NaOH) is a strong base used in many industrial processes. It is manufactured through electrolysis of a sodium chloride solution. The major processes are the mercury cell process, Nelson diaphragm cell process, and membrane cell process. NaOH is used to make soap through saponification, for cleaning, in aluminum production, and to make cryolite. It has health risks as a strong base that can cause burns and damage tissues. Environmental impacts include raising the pH of water.
Sulfuric acid by Rehman Ali Sajjad.
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Understanding 8.5 Acid deposition
Acid deposition occurs when sulfur dioxide and nitrogen oxides emitted from the burning of fossil fuels react with water, oxygen, and other chemicals in the atmosphere to form acids. These acids can fall to Earth as rain, snow, fog or dry particles. Natural processes also produce acid deposition, but human activities such as burning coal and oil have increased acid deposition levels. Acid rain has a pH lower than 5.6 and can damage sensitive forests and lakes. The main pollutants that cause acid rain are sulfur dioxide and nitrogen oxides.
Lecture #3,4 (1).PPT
The document provides an overview of the production of nitric acid. It discusses the history of ammonia production via the Haber-Bosch process and the development of the Ostwald process for producing nitric acid using ammonia as a feedstock. The Ostwald process involves three steps: catalytic combustion of ammonia to produce nitric oxide, oxidation of nitric oxide to nitrogen dioxide, and absorption of the gases in water to produce nitric acid. Higher concentrations of nitric acid can be achieved through direct or indirect processes. The largest uses of nitric acid are in fertilizer production and for manufacturing chemicals.
Sulfuric acid Industries
Lecture Slides by Prof. Imitaz Ali at Ghulam Ishaq Khan Institute for Engineering Sciences and Technology (GIKI).
Nitic Acid.pptx
This document provides information about nitric acid, including its physical and chemical properties, uses, manufacturing process, and production in Pakistan. It describes nitric acid as a colorless liquid used to make fertilizers, dyes, and explosives. Three common industrial methods for producing nitric acid are outlined - the Chile saltpeter method using sodium nitrate, Birkeland-Eyde's method using air, and Ostwald's method using ammonia. Safety precautions for handling nitric acid and first aid measures for exposure are also summarized.
Samical : Unit Processes (part 1)
Here, You will get know about the connection of chemistry and chemical engineering. It is first part of the Unit Process series. In this part I am covering Unit Process like Combustion, Oxidation, Causticization, Nitration and Isomerization.
P block elements
This ppt covers a part of the ncert class 12 chap-7 p-block elements.It covers the group-16 elements in it, like oxygen, sulphur.
P block elements
This ppt covers a part of the ncert class 12 chap-7 p-block elements.It covers the group-16 elements, oxygen, sulphur. If you like please like, share.
Module 2 Revision
The document summarizes several industrial chemical processes:
1) The Haber process produces ammonia from nitrogen and hydrogen at 300 atmospheres of pressure, 450°C, using an iron and potassium hydroxide catalyst.
2) Ammonia is converted to nitric acid in the Ostwald process at 10 atmospheres, 900°C, using a platinum-rhodium catalyst.
3) Sulfuric acid is made via the Contact process, reacting sulfur dioxide with oxygen at 430°C and 2 atmospheres using a vanadium pentoxide catalyst.
4) Aluminum is extracted through electrolysis of aluminum oxide dissolved in molten cryolite.
H2 S and SO2 removal and possible valorization
H2S is a common pollutant in gas and air. This presentation is a review of different techniques to remove H2S ,and possible ways of valorization to sulfuric acid via SO2.
Sulphur (1).pdf
Sulphur dioxide can be prepared in the laboratory by adding dilute sulphuric acid to sodium sulphite. This produces sulphur dioxide gas along with sodium sulphate and water. Sulphur dioxide can be detected using acidified potassium dichromate solution, which turns from orange to green upon reaction. Excess sulphur dioxide bubbled through sodium hydroxide forms sodium hydrogen sulphite. Sulphur dioxide is used to manufacture sulphuric acid via the contact process, where it is oxidized to sulphur trioxide and absorbed in concentrated sulphuric acid.
Unit 01 - HCl HNO3 H2SO4 (1).pptx
The document summarizes common industrial processes for producing hydrochloric acid, nitric acid, and sulfuric acid.
For hydrochloric acid, chlorine and hydrogen gases are reacted and passed through a burner nozzle into a graphite combustion chamber where they ignite to form hydrogen chloride gas. This gas is then cooled and absorbed in water to produce hydrochloric acid.
Nitric acid is produced via the Ostwald process where ammonia is oxidized to nitrogen monoxide, then to nitrogen dioxide, which is absorbed in water to form nitric acid.
Sulfuric acid is made via the contact process where sulfur is burned to form sulfur dioxide, which is further oxidized to sulfur trioxide then reacted with
Hydrogen gas
The document discusses the introduction, preparation, and properties of hydrogen gas. It begins by introducing hydrogen and how it was first artificially produced. It then discusses various methods of preparing hydrogen gas, including the reaction of metals with acids or water, electrolysis of water, and from hydrocarbons like methane. The document outlines the process for producing hydrogen from methane, including desulfurization, reforming, shift reactions, and methanation. It concludes by discussing the physical and chemical properties of hydrogen gas and its various industrial uses such as in rockets, fuel cells, and ammonia production.
Nitrogen.pdf
Nitrogen and its compounds can be prepared through several laboratory methods. Nitrogen gas can be obtained by removing oxygen from air using heated copper turnings, leaving only nitrogen. Ammonia gas is commonly prepared by heating a mixture of ammonium chloride and calcium hydroxide. Ammonia is generally unreactive but will burn or react with substances like oxygen, hydrogen chloride, and metals/metal oxides. It is widely used to manufacture fertilizers and explosives.
Air and water
The document provides information about various chemistry concepts related to air and water:
- It describes chemical tests to identify water and the purification of water supplies through filtration and chlorination.
- The composition of clean air is described as 78% nitrogen, 21% oxygen and small quantities of other gases. Common air pollutants like carbon monoxide and their sources are stated.
- Fractional distillation is outlined as the process used to separate oxygen and nitrogen from liquid air based on their different boiling points.
- Rusting is described as a reaction between iron, air and water that can be prevented by methods like painting and galvanizing to exclude oxygen.
9.1,9.2
The document discusses the manufacture of sulphuric acid, ammonia, alloys, synthetic polymers, glass and ceramics. Sulphuric acid is manufactured through the contact process involving combustion of sulphur to produce sulfur dioxide, oxidation of sulfur dioxide to sulfur trioxide and absorption of sulfuric acid. Ammonia is manufactured through the Haber process involving reaction of nitrogen and hydrogen gases at high pressure and temperature over an iron catalyst. Common alloys include steel, brass and bronze which have improved properties compared to pure metals. Synthetic polymers are long chain molecules formed by polymerization and include plastics such as polyethylene, PVC and nylon. Glass is made mainly from silica while ceramics such
class-xChemical reaction corrosion and rancidity
it is too informative and it is use ful board examination preparation. it is also used as revision slides and remedial classes
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Nitric acid
- 2. OSTWALD PROCESS • Ostwald process is the industrial process used to manufacture nitric acid on a large scale. • Conditions: i. Temperature = 850 - 900o C ii. Pressure = 5 atm iii. Catalyst = Platinum and Rhodium iv. Raw materials = Ammonia and oxygen gas 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g) • Hot copper wire also can catalyze the reaction.
- 3. • In the next step, the NO reacts with oxygen to produce NO2. 2NO(g) + O2(g) 2NO2(g) Then, NO2(g) reacts with water to produce nitric acid (HNO3) and NO. The nitric acid is separated by distillation, and the NO can be recycled through reaction . 3NO2(g) + H2O(l) 2HNO3(aq) + NO(g)
- 4. Uses of nitric acid •To produce ammonium nitrate, one of the most important is to forms nitrogen fertilizers. 3NH3(g) + HNO3(l) 2NH4NO3(s)
- 5. Thank you
- 6. Thank you