RUBBER VULCANIZING ACCELERATOR ·ETU(NA-22)

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Tianjin
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TT OR LC
Min Order Qty:
25 m.t.
Supply Capability:
12000 m.t./month

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Product Description:

 RUBBER VULCANIZING ACCELERATOR ·ETU(NA-22)

 

Chemical Name: Ethylene thiourea
Molecular Formula: C3H6N2S              
 Molecular Weight: 102.17
CAS NO. : 96-45-7
Executive standard: HG/T2343-92 
Specification: 

Item

Index

Top Grade

First grade

Qualified Grade

Appearance
(Visual inspection)

white powder 

 Initial M.P, oC        ≥

195.0

193.0

192.0

Loss on drying, %   ≤

0.30

0.30

0.50

Ash, %                  ≤

0.30

0.30

0.50

Residues on 150μm sieve, % ≤               

0.50

0.10

0.10

Properties: White powder. Little bitter. Density is 1.42-1.43. Soluble in wateralcohol, ethylene glycol and pyridine, do not dissolve ether, benzene, chloroform and petroleum ether.  No pollution to final products. Stabilization storage

Application:: The product can be used to chloroprene rubber, Epichlorohydrin rubber, chlorinated polyethylene, etc., are particularly suited to non-curing system of the chlorine-butylamine Hopewell accelerator. Can often 100-500 oC , with the right selection system can be the best rapid curing, and the whole parade security. Its products vulcanized high tensile strength, permanent deformation small for W (54-1 type polychloroprene), a non-curing system into effect significantly. It usually with zinc oxide and magnesium oxide together with the use, mainly for industrial products, and coating lines, shoes and other clothing chloroprene rubber products.

Packaging: 25kg plastic woven bag, paper with plastic film bag, Kraft paper bag.

Storage: To keep the bags tightly closed in a cool, well-ventilated place at 25 max, to place the goods on the dry wooden shelf at a height of 500px min. And to avoid from moisture, sunshine, light and fires. The recommended max.shelf life is 2 years. 

Note: The product could be ultra fine powder based on customer accurate require. 


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Q:why are catalysts never used up during reactons?
Catalysts facilitate the reaction. They might work in several ways. Here is an example: Catalysts generally react with one or more reactants to form intermediates that subsequently give the final reaction product, in the process regenerating the catalyst. The following is a typical reaction scheme, where C represents the catalyst, X and Y are reactants, and Z is the product of the reaction of X and Y: X + C → XC (1) Y + XC → XYC (2) XYC → CZ (3) CZ → C + Z (4) Although the catalyst is consumed by reaction 1, it is subsequently produced by reaction 4, so for the overall reaction: X + Y → Z They might also just increase the surface area, thus speeding up the reaction. Example: Coke looses its fizz over time if left with the cork unscrewed. This is because the HCO3 is released as CO2. If you drop a menthos into the coke, it explodes with CO2, because the methos is full of tiny dents in the surface (thus giving it a massive surface area). (i blatantly copied the first example from the wiki)
Q:The role of catalyst in chemical reactions
The role of the catalyst is to change the reaction required to achieve the activation energy, can reduce the activation energy is called positive catalyst (that is, usually the meaning of the catalyst), to improve the activation energy is negative catalyst
Q:What kind of chemical reaction requires a catalyst?
Too much reaction, and basically related to the industry
Q:The chemical equation of heating reaction of benzene and hydrogen under the action of catalyst
C6H6 benzene + 3H2 - (arrow) C6H12 cyclohexane (Ni catalytic heating)
Q:Does all chemical reactions have a catalyst?
Not some reaction without catalyst
Q:What is the difference between biological enzymes and chemical catalysts?
Chemical catalysts are widely used, generally the majority of transition elements
Q:how a catalyst can provide a new route in forming the product?
A catalyst may provide a new route in forming a product. Often the reactants have too much energy and bounce off of each other forming few products. The catalyst may provide a surface where the reactants can settle momentarily in close proximity completing the reaction at an increased rate. The catalyst has been pictured (for illustration only) as a surface filled with grooves and when the reactants settle within the grooves (forming a film?) they are close enough to react rather than bounce off of each other. As such the catalyst facilitates the reaction without being used up in the reaction. The catalyst may become 'poisoned' with other molecules that interfere with the desired reaction and the reactants may have to be relatively pure to protect the catalyst.
Q:About chemical catalysts
A catalyst is a substance that accelerates the reaction rate of other reactions and whose quality and chemical properties do not change. Sometimes the catalyst can also participate in the reaction. The elemental iodine in the title is the catalyst for the decomposition of hydrogen peroxide.
Q:Why are enzymes classified as organic catalysts?
A catalyst is a compound that participates in and increases the rate of a chemical reaction without being chemically altered itself. These reactions can be anything from inorganic reactions in fuel cells facilitated by metal catalysts, to the breakdown of glucose in cells by a series of biological catalysts. Biological catalysts operate in biological systems made up of organic molecules (and are made up of organic molecules themselves - mostly carbon)... thus it's logical to think of enzymes as organic catalysts.
Q:how do catalysts help in green chemistry?
Catalysts reduce the energy barrier for reactions, meaning they require less energy to make the forward reaction go. This means less heat, light, or other energy sources are required to perform the same reaction without a catalyst. Also, by definition, a catalyst is not consumed in a reaction and can therefore be recycled many many times before replacement is necessary.

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