RUBBER VULCANIZING ACCELERATOR TMTD (TT)

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

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Product Description:

RUBBER VULCANIZING ACCELERATOR TMTD(TT) 

 

Chemical Name : Tetramethyl thiuram disulfide
 Molecular Formula: C6H12N2S4
 Molecular Weight: 240.43
CAS NO. : 137-26-8
Executive standardHG/T 23342007 
Specification: 


Item 

Index

First-class products

Acceptable end-product

Appearance
(Visual inspection)


White, light gray powder or granular 

 Initial M.P, oC             ≥ 

142.0

140.0

Loss on drying, %          ≤ 

0.30

0.30

Ash, %                        ≤ 

0.30

0.30

Residues on 150μm sieve, %                           ≤ 

0.00

0.10

Properties: White, light gray powder or granular. The density is 1.29. Soluble in benzene, acetone, chloroform, CS2 partly soluble in alcohol, diethyl ether, CCI4 insoluble in water, gasoline and alkali with lower concentration. Meeting hot water becomes to dimethylamine  ammonium and CS2. Be sensitive to skin and pneogaster

Application: Can be used as a single accelerator, as a secondary accelerator or as a sulphur donor in most sulphur-cured elastomers. Scorchy and gives fast cure rates. Produces an excellent vulcanisation plateau with good heat aging and compression set resistance in sulphurless and EV cure systems Good color retention is obtained in non-black vulcanisation. A valuable secondary accelerator for EPDM. May be used as a retarder in the vulcanisation of polychloroprene rubber with ETU and also be used as bactericide and pesticide

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

Storage: The product should be stored in the dry and cooling place with good ventilation, avoiding exposure of the packaged product to direct sunlight. The validity is 2 years.

Note: The product could be ultrafine powder based on customer accurate requirement.

 

 


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Q:Is the chemical reaction rate constant related to the amount of catalyst used?
The decomposition of hydrogen peroxide, manganese dioxide in addition to the catalyst, but also in which it can be considered a carrier (from the surface of manganese dioxide to emit small bubbles, you should be able to see), so the amount of more than certainly can speed up the reaction.
Q:What is chemical adsorption and its relationship with heterogeneous catalysis
The catalytic cycle includes five steps: diffusion, chemical adsorption, surface reaction, desorption and reverse diffusion.The chemical adsorption is an important part of the heterogeneous catalysis process, and the adsorption of the reactants on the catalyst surface,
Q:Can you describe at least 4 ways a catalyst can lower the activation energy of a reaction?
To see how a catalyst accelerates the reaction, we need to look at the potential energy diagram shown below which compares the non-catalytic and the catalytic reaction. For the non-catalytic reaction, the figure is simply the familiar way to visualize the Arrhenius equation: the reaction proceeds when A and B collide with succificient energy to overcome the activation barrier. The change in Gibbs free energy between reactants, A + B, and the product P is delta G. The catalytic reaction starts by bonding of the reactants A and B to the catalyst, in a spontaneous reaction. Hence, the formation of this complex is exothermic and the free energy is lowered. There then follows the reaction between A and B while they are bound to the catalyst. This step is associated with an activation energy; however, it is significantly lower than that for the uncatalyzed reaction. Finally, the product P seperates from the catalyst in an endothermic step. The energy diagram illustrates 4 ways the catalyst works : The catalyst offers an alternative path for the reaction that is energetically more favorable The activation energy of the catalytic reaction is significantly smaller than that of the uncatalyzed reaction; hence the rate of the catalytic reaction is much larger The overall change in free energy for the catalytic reaction equals that of the uncatalyzed reaction. Hence, the catalyst does not affect the equilibrium constant for the overall reaction. A catalyst cannot change the thermodynamics of a reaction but it can change the kinetics. The catalyst accelerates both the forward and the reverse reaction to the same extent. In other words, if a catalyst accelerates the formation of product P from A and B, it will do the same for the decomposition of P into A and B.
Q:What is a chemical catalyst?
A substance that participates in chemical reactions but does not change the quality and chemical properties. It can change the reactant activation energy, speed up or slow down the reaction rate.
Q:A catalyst?
Always speeds the reaction rate.
Q:Why can the catalyst change the chemical reaction rate?
Change the course of the reaction
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
Q:why are enzymes called catalysts?
Because they speed up chemical reactions by lower the amount of energy required to start the reaction (called activation energy). A catalyst is something that speeds up a reaction - which is what enymes do.
Q:What is the microcosmic principle of the catalytic reaction in the chemical reaction?
It is actually directly involved in the reaction, but, after the reaction, it has become a product out, the equivalent of no response
Q:High school stage chemical catalyst
High school is the most common is manganese dioxide, and potassium permanganate heating oxygen, hydrogen peroxide decomposition are used, which is inferred in the problem there is a lot of

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