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FAQ
- What is the principle of the catalyst? Why can change the rate of chemical reactions and their own without any change
- The catalyst is a substance that alters the reaction rate without changing the total standard Gibbs free energy of the reaction. The composition, chemical properties and quality of the catalyst itself do not change before and after the reaction; its relationship with the reaction system is as highly selective (or specific) as the relationship between the lock and the key. A catalyst does not catalyze all chemical reactions. For example, manganese dioxide catalyzes the thermal decomposition of potassium chlorate, accelerates the reaction rate, but does not necessarily have a catalytic effect on other chemical reactions. Some chemical reactions are not only the only catalyst, such as potassium chlorate can be thermally decomposed in the catalytic role of magnesium oxide, iron oxide and copper oxide, etc., potassium chlorate oxygen can also be used when the red brick powder or copper oxide as a catalyst.
- Please make it simple because I need it for school and please give to examples for the second part Thanx :D
- A catalyst is a substance that speeds up the rate of a chemical reaction with itself being chemically unchanged at the end of the reaction. They are useful as they help to lower the minimum amount of energy needed ( also known as activation energy) to start the reaction. Hence, by lowering the activation energy of the reaction, they help to speed up the rate of reaction. For example, in the Haber process for the manufacture of ammonia, the catalyst iron is added to speed up the rate of reaction between hydrogen gas and nitrogen gas. Otherwise, the reaction would have proceeded much more slowly. Another example is the catalyst nickel used in the manufacture of margarine and vanadium (V) oxide for manufacturing sulfuric acid. As catalyst remain chemically unchanged after a reaction, they can be reused again and hence, they are required in minute amounts. An example is the washing powder used in washing clothes, they help to remove food stains by digesting the proteins in food. They can be reused after each reaction and hence, you do not need to add in the whole packet of washing powder but only a few spoonful.
- The role and significance of chemical catalysts
- The catalyst does not participate in the reaction, but only acts as a catalyst, and finally gets the catalyst composition unchanged. But if the catalyst, your reaction will be very slow or even not happen.
- about 1-3 sentences on this will do thank you
- 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.
- Is the chemical reaction rate constant related to the amount of catalyst used?
- In fact, the catalyst is to participate in the reaction (junior high school textbooks do not respond is to allow students to understand), but the reaction to the final return to the original state.
- Can a catalyst react with a reactant?
- Catalysts are of different categories. There are some reactions, in which only the presence of some compound increases/decreases the rate of the reaction. In other examples, the catalyst do react with the reactants and provide a different path for the reaction. The product is formed and the catalyst is recovered. Not even a single molecule is consumed after the reaction. But if you take a sample while the reaction is going on, you might find a decrease in the concentration of the catalyst. (An example is the use of Mangnese dioxide (MnO2) in the conversion of Potassium Chlorate (KClO3) to Potassium Chloride and oxygen. The MnO2 added at the initiation of the reaction is in form of crystals and at the end of the reaction it is recovered as finely divided powder. This simply shows that MnO2 reacted with KClO3 initially and finally got detached in form of a powder.)
- CO and NO react under the action of a catalyst to generate chemical formulas for CO2 and N2.
- C from +2 to +4 price 2e * 2
