SDIC In Water Treatment Chemicals by Granular Tablets Powder

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SDIC Introduction:

SDIC  White powder or grain with chlorine odor . It is a strong oxidant and chlorate agent and can dissolved in water easily . Its aqueous solution assumes weak acidity and the active chlorine in its dry products lose little when it is stored for a long time at the atmospheric temperature .

Quick dissolving tablet within 10 minutes. It is used in hospital, hygienic, disaster protection, food industry, and aquaculture etc.

The tablet have 0.5g, 1.0g, 3.3g, 5g, 7g, 10g.

Packed in 100g, 500g, 1kg, 2kg, 3kg & 5kg plastic bucket.

And we can supply tablet form: 1g, 2.7g, 3.3g, 3.5g, 5g, 10g & 20g.Package: in 500g, 1kg, 2kg, 5kg or do with customer requirements

SDIC Imange:

SDIC In Water Treatment Chemicals by Granular Tablets Powder

SDIC Specification:

Chemical Name

Sodium Dichloroisocyanurate

Molecular Formula:


Molecular Weight:


CAS Number:





Available chlorine(%,min)



Moisture content(% max)



PH Value(1% solution)



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Main usage:
this products can effectively kill various germs, fung uses and viruses, specially A&B type hepatitis viruses. It is effective on killing algae, decolorizing cleaning water or bleaching .It can be widely used for epidemic prevention, livestock farming , industry and agriculture.





SDIC In Water Treatment Chemicals by Granular Tablets Powder

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Q:Several experiments were carried out using catalysts
Hydrogen peroxide in the manganese dioxide as a catalyst for decomposition reaction: 2H2O2 == MnO2 == 2H2O + O2 ↑ (laboratory oxygen principle)
Q:Pls help me define a catalyst.?
A substance which speeds up or slows down a reaction without taking part in it.
Q:Chemical catalyst system baa?
Catalyst is divided into inorganic catalyst and organic catalyst organic reaction generally need more catalyst, such as concentrated sulfuric acid
Q:Chemical catalyst
Catalyst before and after the reaction of the same quality,
Q:Chemical reaction plus catalyst on the △ H no effect
Since the addition of the catalyst only accelerates the reaction process and does not have an effect on the reaction product and the reactants
Q:What happens to the rate of a reaction when the concentration of a catalyst is doubled?
A catalyst speeds up a chemical reaction by providing an alternate reaction pathway with a lower activation energy, thus increasing the number of collisions that can result in the formation of product. When the catalyst is a reactant in the rate determining step, and the reaction is first order in the catalyst, then a doubling of the concentration will double the rate. But if the rate determining step which includes the catalyst is not first order, then doubling the concentration won't double the rate. Then there is the case of a heterogeneous catalyst in which the reaction is essentially zero order in the catalyst. The amount of catalyst won't affect the speed of the reaction beyond the initial increase. The mere fact that the catalyst is present speeds up the reaction.
Q:In chemistry what is a catalyst and an example?
Catalysts are substances that increase the rate of a reaction by providing a low energy shortcut from reactants to products. In some cases, reactions occur so slowly that without a catalyst, they are of little value. Nearly all reactions that occur in living cells require catalysts called enzymes- without them, life would be impossible. There are two important classes of catalysts: homogenous catalysts like enzymes and aqueous ions that are uniformly mixed with the reactants, and heterogeneous catalysts that provide a surface that holds and reconfigures the reactants in a way that is favorable for reaction. Examples of homogeneous catalysis. Catalysts in solution with the reactants usually provide fast reaction paths by allowing reactants to form an unstable intermediate that quickly decomposes into products. For example, the substitution reaction CH3CH2OH(g) + HCl(g) H2SO4 ----->CH3CH2Cl + H2O(ell) is catalyzed by acid because the ethanol is converted into unstable CH3CH2OH2+, which quickly reacts with Cl- to produce the products. Definition: A catalyst is a subtance that increases the rate of a chemical reaction by reducing the activation energy, but which is left unchanged by the reaction. Examples: A piece of platinum foil is a catalyst for the combustion of methane in air.
Q:Chemical reactions in the presence of impurities will cause catalyst poisoning
In fact, the magazine and the catalyst reaction, making the catalyst deterioration or activity decreased
Q:What is the similarity between enzymes and general chemical catalysts?
(1) The enzyme is the same in many respects as a biocatalyst and a general catalyst, such as a small amount and a high catalytic efficiency. As with the general catalyst, the enzyme can only change the rate of chemical reaction and does not change the equilibrium of the chemical reaction It is possible to catalyze the activation of a large number of substrates in a short time and to reflect the high efficiency of enzyme catalysis.The enzyme can reduce the activation energy of the reaction (activation) (△ G) during the reaction, but the reaction rate is accelerated and the reaction time is reduced, but the equilibrium constant is not changed. (2) However, the enzyme is a biological macromolecule (1) Enzyme-catalyzed high efficiency: The catalytic effect of the catalyst can increase the reaction rate by 10 ^ 6 ~ 10 ^ 12 times, which is at least several times higher than that of the conventional catalyst. (2) The enzyme catalyst Highly specificity: including specificity of response, substrate specificity, chirality specificity, geometric specificity, etc., that an enzyme can only act on a certain class or a specific substance. Bond, ester bond, peptide bond and so on can be catalyzed by acid-base hydrolysis, but the hydrolysis of these chemical bonds are different, respectively, the corresponding glycosidase, esterase and peptidase, that is, they were specific (3) enzymatic reaction conditions are mild: enzymatic reaction is generally carried out in aqueous solution of pH = 5 ~ 8, the reaction temperature range is 20 ~ 40 ℃
Q:Explain, using an example, how a heterogeneous catalyst works?
Because of the production of photochemical oxidants from NOx reacting with hydrocarbons in sunlight Noxer blocks are used to rid the NOx from the surroundings through The titanium dioxide (TiO2) on the bocks absorbs ultra-pink radiation from daylight which excites its electrons to a bigger orbital. On the outside of the crystals of TiO2 a reaction happens between oxygen and a high power electron from the TiO2. O2 + e־ --O2 ־ The excessive vigor electron is then given back to the TiO2 when water then reacts with the oxygen to present H2 O + O2 --H+ + O2 ־ + OH Nitrogen dioxide is oxidised to nitrate ions as a result of the hydroxyl radical being an awfully strong oxidising agent NO2 + OH --H+ + NO3 ־ The superoxide from response 3 also varieties nitrate ions from nitrogen monoxide. NO + O2 ־ --NO3 ־ This nitrate is washed away through rain or combines with the concrete within the block.

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