User:Mountainninja

Works
Mostly working on Chemistry articles.

Expands Trimer (chemistry) with 10 examples and edit related links and articles from sources in English Wikipedia, German Wikipedia and Polish Wikipedia -- Mountainninja (talk) 23:15, 4 May 2014 (UTC)

/draft

1.1
Elegance of the peroxide processing of ammonia in making hydrazine, hydroxylamine, hyponitrous acid ?

Not co-producing salt(s) in this process aside, its role of acetone fixating and protecting the ammoniacal nitrogen atom so a hydrogen-nitrogen bond can participate in substitution and an carbon-nitrogen double bond addition reaction. The 3,3-disubstitutedoxaziridine can be used for: 1condensation reaction with more ammonia, as in the peroxide process for hydrazine. 2hydrolysis, giving hydroxylamine Ketazine is formed in the process, 3Yet more hydrogen peroxide can react with, to gives hyponitrous acid. As this ketazine-lysis takes two oxygen atoms, can even dioxygen molecule from purified air be a reactant, thus saving hydrogen peroxide ? I doubt. Thus, all these three compounds can be viewed essentially as oxidation products of ammonia by hydrogen peroxide.

2
Salts of various sulfur oxoacids can be made from sulfur acid exhaust during the contact process. Bubbling excess sulfur dioxide through a solution of suitable base, such as sodium hydroxide, produces sodium bisulfite.
 * + NaOH  →

Evaporating a solution of sodium bisulfite saturated with sulfur dioxide leaves the product sodium metabisulfite behind:
 * 2 − ⇌ H2O + S2O52−

Sodium dithionate is prepared from the reactions between sodium bisulfite with either manganese dioxide, silver oxide, chlorine or solution of sodium hypochlorite. All these reactions generate byproducts that are needed to be separated and not regenerated in the reaction. The following reactions would deviate from the traditional routes: Disproportionation of solid sodium metabisulfite generates sodium dithionite whose melting point is 52°C and sodium dithionate 190°C. By careful hitting of
 * 2 S2O52− →  S2O42−  +  S2O62−

Or, sodium thiosulfate is produced on an industrial scale chiefly from liquid waste products of sodium sulfide or sulfur dye manufacture. Oxidizing thiosulfate by adding one oxygen atom at a time to each thiosulfate can generate the desired salt of sulfur oxoacid from dithionite, metabisulfite and dithionate in individual pots of reactions.
 * Pot 1: S2O32− +  [O]  →  S2O42−
 * Pot 2: S2O32− +  2[O]  →  S2O52−
 * Pot 3: S2O32− +  3[O]  →  S2O62−

Can heteropoly acids such as catalyze these oxidations of solid sodium thiosulfate? For reference, silicotungstic acid has been commercialized for the oxidation of ethylene to acetic acid:
 * C2H4 +  O2   →   CH3CO2H

Analogously,
 * Pot 1: S2O32− +  H2O2 (Phosphomolybdic acid) →  S2O42− + H2O
 * Pot 2: S2O32− +  O2 (silicotungstic acid)  →  S2O52−
 * Pot 3: S2O32− +  O3 (silicotungstic acid) →  S2O62− or S2O32−  +  H2O2 +  O2 (Phosphomolybdic acid) →  S2O42− + H2O

3

 * Hydroformylation of carbon dioxide in supercritical or STP conditions yields glyoxylic acid: this synthesis creates a pathway to convert unused industrial gas or desulfurized and cleaned flue gas into biodegradable products or merchandise. Hydrogen, carbon monoxide and   can also come from plasma gasification(PG) of municipal solid waste(MSW). In essence, the proportion between burning syngas for electricity generation and manufacturing biodegradable products can be balanced to different needs of industry, commerce and communities.


 * Regarding PG and its commercialization, unused syngas and exhaust of energy generation can be converted to biodegradable products such as glyoxylic acid and the carbon dioxide and steam therein can be pressured into supercritical conditions to leach metal ions from the slag in PG before vitrification.


 * Instead of FIRST vitrifying the slag byproduct, could metal be first recovered before the vitrification ? For example, ADEQUATE AMOUNT of scrap aluminum and aluminium dross sacrificed by adding to the waste UPSTREAM so elements below aluminum on the reactivity series are reduced to metal when all inorganic materials are vitrified. The metal being denser than slag, can be recovered by centrifugal separation. Obviously, aluminum can reduce silica to produce silicon and the purpose of adding aluminum is to recover some other metals, say copper; so only adequate amount of scrap aluminum is needed. -- Mountainninja (talk) 23:32, 26 September 2014 (UTC)

Ideas for thought: Fractional crystallization (chemistry) Betterton-Kroll process Betts electrolytic process Parkes process -- Mountainninja (talk) 15:20, 19 February 2015 (UTC)

3.1

 * Supercritical carbon dioxide and water treatment on lignosulfonates, tall oil and turpentines from sulfate and Kraft processes may yield syngas. As unused or exhaustive carbon dioxide, carbon monoxide, hydrogen gases are synthesized to glyoxylic acid, the acid can also be added into supercritical fluid to increase its hydrogen content. At any rate syngas is produced and thus synthesized into organic products thru common gas to liquids industrial procedures.

4
Can decomposing sulfamic acid with catalyst be a novel preparation of hydroxylamine ?

The would-be byproduct sulfur dioxide is recycled for preparing more sulfamic acid, sulfur trioxide, sulfuric acid or oleum. In essence this novel synthesis eliminates the use of chlorine and ammonia compounds and links more closely the industries for sulfuric acid and urea preparation.

5
Chloralkali process, Solvay process, alkali metals, alkaline earth metals manufactures

Can carbon dioxide be pumped into sodium hydroxide product from the Chloralkali process to precipitate all formed sodium bicarbonate due to common ion effect in the brine ?

Besides manufacturing sodium bicarbonate and sodium carbonate, desired concentration of pure sodium hydroxide is re-manufactured by dissolving appropriate amount of sodium oxide into water, with heat recovery apparatus available for further heating of more sodium bicarbonate. Note that pure alkaline earth metal carbonates can be manufactured by reacting sodium carbonate with alkaline metal chlorides.

Pure sodium chloride can then be manufactured by reacting the pure sodium hydroxide with the pure hydrogen chloride from reacting hydrogen and chlorine products from the chloralkali process.

This pure sodium chloride can then be used for electrolysis for sodium metal. Thus the Chloralkali process is both synthesis and refining processes. Note that no ammonia is used, in contrast to usage in the Solvay proces, and no mercury is used in contrast to usage in the Castner–Kellner process. Pure alkaline earth metal chlorides can also be manufactured in similar processes for electrolysis for alkaline earth metals.

6.1
Nitrogen oxides byproducts from nylon manufacturing can all be converted to nitrogen monoxide. It is then reacted with adipic acid to form N-oxoadipamide, that is later hydrogenated to hexamethylenediamine.

+ → 3 3 +  →   +  8 →  + 4

In essence, nitrogen oxides byproducts can be reprocessed and then reacted with cyclohexene or cyclohexane to cyclohexanone and/or cyclohexanol; nitrogen gas and water are byproducts instead of nitrogen oxides.

6.2
is used to generate anhydrous metal nitrates from the oxides:


 * MO + 3 →  + NO

How about reacting the organic impurities and oxides of nitrogen with alkali metal and/or alkaline metal carbonates into inorganic nitrates, carbonate esters and compounds of nitrogen that do not normally form salt, such as nitrous oxide. Because of the polar and nonpolar nature of these liquids and solids, they can be separated by distillation, fractional distillation and recrystallization. Both group of ionic and covalent compounds can be commercial sources of chemicals. Using alkali metal carbonates show two advantages. Explosive risks need to be taken by simply combining the organic impurities and oxides of nitrogen into nitrate esters; carbonate esters do not pose such risks. Alkali metal carbonates can be manufactured from chloralkali process, in which carbon dioxide is to react with the sodium hydroxide product to form sodium carbonate. Thus the recycling and reuse of nylon manufacture byproducts, chloralkali process, alkali metal carbonates manufacture, alkali metals manufacture can be combined into one greater manufacturing industry.

6.3
Nitrous oxide can still be used for such as oxidation of benzene to phenol, or oxidation of ammonia to hydroxylamine, which is useful in the Beckmann rearrangement of cyclohexanone oxime to caprolactam in the manufacturing nylon 6.

+ →  +

Hydrogenation of nitric oxide dimer to hyponitrous acid, and more hydrogenation to hydroxylamine.

+ →
 * 2 +  → 2

Nitric oxide reacts in free-radical addition to hydrogen sulfide with elimination of water to tetrasulfur tetranitride.

+ -  →

and so on...

Nitric oxide(NO) or NOx reacts on commercial metal sulfide ores to yield metal oxides and tetrasulfur tetranitride, which can be decomposed into nitrogen gas and sulfur. S4N4 itself can be an reagent introducing sulfur into chemical compounds. Also NO is one of the NOx. So in essence, the reaction converts three environmental problematic compounds to two other more valuable products.

Ideas for thought: Herz reaction Sulfilimine Sulfamide

6.4
Dinitrogen monoxide replaces silver oxide as a mild oxidizing agent. For example, as is a by-product of manufacturing nylon which uses hydroxlamine,  can be used to oxidize ammonia to yield hydroxylamine and dinitrogen which is recycled. + →  +

7
Condensation and dehydration of acrolein and acetonitrile afford pyridine. + -  →

Acetonitrile is a byproduct from the manufacture of acrylonitrile. Most is combusted to support the intended process but an estimated several thousand tons are retained for the above-mentioned applications.

Acrolein is prepared industrially by oxidation of propene. The process uses air as the source of oxygen and requires metal oxides as heterogeneous catalysts: + →  +

Useful template
Template:Clear