RUBBER VULCANIZING ACCELERATOR NOBS (MBS)

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Tianjin
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25 m.t.
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12000 m.t./month

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Product Description:

RUBBER VULCANIZING ACCELERATOR NOBS(MBS)

Chemical NameN-Oxydiethylene-2-Benzothiazole Sulfenamide
 Molecular formula: C11H12N2S2O
 Molecular Weight:253.35
CAS NO. : 102-77-2 
Executive standardGB/T 8829-2006
Specification: 


Item 

Index

High-class products

First-class products

Acceptable end-product

Appearance
(Visual inspection)

Faint yellow or orange granules 

Initial M.P, oC        ≥ 

81.0

80.0

78.0

Loss on drying, %     ≤ 

0.40

0.50

0.50

Ash, %                    ≤ 

0.20

0.30

0.40

Insoluble in Methanol%        ≤

0.50

0.50

0.80

Free amine,%        ≤ 

0.50 

Purity,%                 ≥ 

95.0 

Properties: Faint yellow to brown lamellae. 80°C melting point.soluble benzene; carbon tetrachloride; ethyl acetate; ethanol, soluble in dichloromethane; acetone, less petrol, do not dissolve in water. Heating gradual decomposition. 

ApplicationIt'after-effect quick accelerator. Scorching time is longer and the processing safety is good.

Packing: 25kg paper bag inner with PE bag

Properties: The product should be stored in the dry and cooling place with good ventilation . The product should be avoid hot sunshine. 

 


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Q:In the catalyst and light conditions to break down the water to get the chemical equation of hydrogen
2H2O = 2H2 ↑ + O2 ↑
Q:What is the nature of the chemical catalyst?
Catalyst is the chemical reaction can change the reaction rate of other substances, and its own quality and chemical properties in the chemical reaction before and after the material has not changed Some catalyst can really slow down the reaction rate, the book said only refers to the usual circumstances , In general, junior high school and high school teaching into the do not do special instructions are understood to speed up the reaction rate. It is only necessary to know that the catalyst is not only used to speed up the reaction rate. Once the reversible reaction reaches equilibrium, adding the catalyst does not break the balance, but at the same time accelerates the forward and reverse reaction rates. The degree of acceleration is the same.
Q:Can some chemical reactions have a variety of catalysts that are correct or wrong?
Very correct, many reactions can have a lot of catalyst. Such as hydrogen peroxide decomposition can be used manganese dioxide or fe destroy
Q:What is a catalyst/catalase? help?
an enzyme that decomposes hydrogen peroxide into oxygen and water.a substance that causes or accelerates a chemical reaction without itself being affected. To put thing simply, a catalyst is any substance that speeds up a chemical reaction. These can be natural or manmade. Catalase is actually a specific type of naturally-occuring catalyst, an enzyme in cells that decomposes hydrogen peroxide (Which is extremely toxic to life!) into harmless components. Catalase enzymes are highly concentrated in the aptly named cell organelles known as peroxisomes. Just remember- if the word ends in -ase, it's a type of enzyme! :) Hope this information helps!
Q:Catalyst and Intermediate.?
Cl is the catalyst. ClO the intermediate. The catalyst is the component which does not change in overall reaction. He forms some intermediate component(s) with the reactants. In the later reaction steps the intermediate(s) react forming the catalyst in its original state. (a) The overall order is the sum of the orders with respect to the components: n = 1 +1 = 2 (b) the unit of the rate of reaction is r [=] mol/ (Ls) (more general mol per unit time and volume) compare dimensions mol / (Ls) [=] k · mo/L · mol/L =k [=] L/(s mol) (more general unit volume per unit time and mole) (c) First reaction For elementary reaction steps the order of the reaction rate with respect to a reactant is equal to stoichiometric coefficient. Hence the rate of first reaction is: r₁ = k₁·[Cl]·[O₃] Overall rate is given by the rate determining step, while other reaction steps are in equilibrium: r = r₁ = k₁·[Cl]·[O₃] If second reaction is the rate determine step r₂ = k₂·[O]·[ClO] while reaction 1 is at equilibrium K₁ = ( [ClO]·[O₂] ) / ( [Cl]·[O₃] ) =[ClO] = K₁·( [Cl]·[O₃] ) / [O₂] the overall rate would be: r = r₂ = k₂·[O]·[ClO] = K₁·k₂·[O]·[Cl]·[O₃] / [O₂] = k·[O]·[Cl]·[O₃] / [O₂] That doesn't match the observed rate law
Q:About chemical catalysts
The role of the catalyst is to change the reaction rate of the chemical reaction, which itself does not participate in the reaction! The
Q:A question about the catalyst in a chemical reaction
CuO exothermates when catalyzing the decomposition of hydrogen peroxide, so the reaction becomes faster.
Q:Exemplify the use of green catalysts in green chemistry
How can a green catalyst, they do not react
Q:catalyst..........?
H+ is the ion contained in acids.... When acids are dissolved in water (H+)+(H2O)=H3O+ Both are the same......
Q:Is it not the rate to accelerate the addition of the catalyst to the catalyst, and that is why the balance does not move
In the chemical equilibrium, after adding the catalyst, the positive and negative reaction rate increases equally, but the positive reaction rate is still equal to the reverse reaction rate, so the balance does not move

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