Rubber Chemcials Rubber Antioxidant 6PPD 4020
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6PPD 4020
Chemical Name:N-(1,3-dimethylbutyl)-N'-phenyl-p-phenylenediamine
Molecular Formula：C18H24N2
Molecular Weight:268.40
CAS NO.：793-24-8
Executive standard:HG/T 3644-1999
Specification:
| Index |
| |
Appearance |
|
Soften Point,℃ ≥ | 45.0 |
Loss on drying,% ≤ | 0.50 |
Ash,% ≤ | 0.15 |
Assay（GC）% ≥ | 96.0 |
Solidifying Point,℃≥ | 45.5 |
Properties: Dark brown to dark violet pastilles relative density of 0.986-1.00. Soluble benzene, acetone, ethyl acetate, toluene dichloromethane and slightly soluble in ether, do not dissolve in water. Provides powerful and antioxidant properties with excellent high temperature and flex resistance to rubber compounds.
Applications:Include the use in pneumatic,solidtires,beles,hoses,cables,bushings,automotive mounts and general mechanical products that are exposed to continuous and intermittent dynamic operating conditionsand and require protection from coronations.
Packing:Packed in 20kg per bags.
Properties: The product should be stored in the dry and cooling place with good ventilation. The product should be avoid hot sunshine.
- Q: What is the maximum impact of the chemical reaction rate? Such as catalyst, temperature, concentration. If you can, you can row order.
- Temperature and concentration also depends on the specific circumstances of the situation
- Q: Cl + O3 ---> ClO + O2O + ClO ---> Cl + O2= O + O3 ----> 2O2What is the catalyst? The intermediate?How do you know which is which? If the rate law is rate=k [O3] [Cl]determine:a) the overall order.b) unit for k.c) the rate determining step, justify your answer.
- 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: r? = k?·[Cl]·[O?] Overall rate is given by the rate determining step, while other reaction steps are in equilibrium: r = r? = k?·[Cl]·[O?] If second reaction is the rate determine step r? = k?·[O]·[ClO] while reaction 1 is at equilibrium K? = ( [ClO]·[O?] ) / ( [Cl]·[O?] ) =[ClO] = K?·( [Cl]·[O?] ) / [O?] the overall rate would be: r = r? = k?·[O]·[ClO] = K?·k?·[O]·[Cl]·[O?] / [O?] = k·[O]·[Cl]·[O?] / [O?] That doesn't match the observed rate law
- Q: Chemistry why the catalyst can be equal to speed up the positive reaction rate
- Since the catalyst only changes the activation energy and the amount of reactivity can be reduced, the amount of reaction energy is also reduced. Therefore, a positive catalyst is also a good catalyst for its reaction. Speed up the same multiple.
- Q: Is the catalyst in the chemical reaction better?
- The efficiency of the catalyst is very high, as long as a little bit on it, with too much in addition to increase the cost of meaningless. Positive catalyst can increase the rate of several thousand times. Fast ... I know there will be about a thousand years shortened to 1 second. There are slowdown in the catalyst, people taught not learned. Other versions of the textbook is not clear. Should not learn.
- Q: What kind of chemical substances can seriously damage the ozone layer, as a catalyst or reactants can be?
- Hundreds of years ago the news once the industrial production and emissions of ozone generated less way, the ozone layer will still be thin.
- Q: The beginning of the chemistry plus the catalyst and the plot without the Cuihua agent
- Activated molecular map
- Q: I know that a species that does not appear in the chemical equation may also affect the rate of a reaction - e.g. a catalyst. But does that mean the catalyst can be present in the rate equation, and if so are catalysts always present in the rate equation?
- Yes, a catalyst can be included in a rate law. That's because, most reactions occur in a series of step and the rate is based on the rate determining step, which is the slowest step. A catalyst may be a reactant in the rate determining step, and a product in a subsequent step. Therefore, the catalyst is not included in the overall reaction. But a catalyst need not always be in the rate law. The rate law is usually based on the rate determining step. ========== Follow up =========== In the free response questions on the AP chemistry exam there has been at least one case where a rate law included a catalyst( 2002D). Brown and LeMay always include at least one in their examples, and I always cover this situation when I teach rate laws and mechanisms in AP chemistry. Here is one comment: Other examples of species not in the balanced reaction occurring in the rate law would include catalysis, where a catalyst does not normally appear in the balanced reaction but does appear in the rate law. www.chem.arizona.edu/~salzmanr/48... Consider this generalized reaction which is catalyzed by M A + B --C A + M --Q ... slow Q + B --C ... fast M is the catalyst, and Q is the intermediate. The slow, or rate determining step, depends only on the concentrations of A and M, the catalyst. So even though the overall reaction does not include, M, the rate law does. Rate = k[A][M]
- Q: Especially how can i explain the experiment with a paper and 2 paperclips with the paper acting as the catalyst.
- A catalyst acts on one material to activate it towards reaction with another material that it would not otherwise spontaneously react with (it lowers the reaction's activation barrier). For instance, the 2 paperclips may not want to react with each other, but if the paper attaches to one, it becomes more reactive and it will now clip onto the other paperclip. The catalyst then leaves (paper is detached) which is called catalyst regeneration, which goes on to activate another molecule in the same fashion. A common example is using Lewis acid catalysts to activate carbonyls by coordinating to the oxygen so that the the carbon becomes more electrophilic for attack by some nucleophile.
- Q: give an example of how a catalysts speeds up the rate of reaction?? thank you!!?
- When making margarine, nickel is used to speed up the process.
- Q: Will the catalyst decompose during the reaction between two substances? Exp:the decomposition of hydrogen peroxide.Will the manganese 4 oxide decompose?
- Catalysts are not used/destroyed in any reactions, it merely speeds up the process by lowering the reaction activation energy. It functions by being able to weaken or break the required bonds necessary in the chemical reaction (thus lowering activation energy) through temporary and weak bonding to form a complex. In this case the H2O2 molecule will bind with the MnO2 molecule due to the complimentary sites (thus forming a complex) to weaken the bonds for decomposition, but after decomposition the products (oxygen and water molecules) break off from the catalyst (as there are no more complementary sites with them) thus the catalyst will not be destroyed.
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Rubber Chemcials Rubber Antioxidant 6PPD 4020
- Ref Price:
-
- Loading Port:
- Tianjin
- Payment Terms:
- TT OR LC
- Min Order Qty:
- 25 m.t.
- Supply Capability:
- 12000 m.t./month
OKorder Service Pledge
Quality Product, Order Online Tracking, Timely Delivery
OKorder Financial Service
Credit Rating, Credit Services, Credit Purchasing
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