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Theory of catalytic decomposition of hydrogen peroxide
Catalytic decomposition of hydrogen peroxide introduction
What are the main importances of using catalyst reactions in chemical industries
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CATALYSTS Catalysts are substances used to increase or decrease the rate of a chemical reaction. A catalyst is a substance which alters the rate of a chemical reaction but is chemically unchanged at the end of the reaction.The word catalysts originally comes from the word Catalysis meaning the change in rate of a chemical reaction. Catalysts unlike other substances, may participate in many chemical transformations but never consumed by the reaction itself. This means that, when a catalyst is added to two substances to increase the reaction rate between them, the catalyst isn't consumed and may be used again.([3]"Chem4Kids.com: Reactions: Catalysts and Inhibitors.") For example, the decomposition of hydrogen peroxide; in this chemical reaction , manganese oxide can be used as a catalyst. Using the help of the manganese oxide, the reaction will take place faster but never the less, manganese oxide itself will not be consumed. Catalysts that speed up the rate of reaction are know as positive catalysts and others that slow down the rate of reaction are know as inhibitors or negative catalysts. Scientifically speaking, catalytic reactions are the fastest chemical reactions. The rate of the reaction depends on the frequency of the physical contact of the two reactants. The more they collide, the more activation energy is produced and therefore the faster the reaction. However, although catalysts are not consumed by the chemical reaction itself, they can be inhibited, destroyed or deactivated. But never the less catalysts authorizes a suitable local environment in order to promote one or more chemical reactions to react. ([6]"The Effect of Catalysts on Rates of Reaction." Chemguide) Technically, the importance of catalysts pl... ... middle of paper ... ...ader's CHEM4KIDS.COM. Web. 08 Oct. 2011. . [4]Creative Chemistry - Fun Activities, Worksheets, Games and Revision Quizzes. Web. 08 Oct. 2011. . [5]"Dubai's Traffic Pollution among World's Worst - ArabianBusiness.com." Middle East Business News, Gulf Financial & Industry Events & Information - ArabianBusiness.com. Web. 08 Oct. 2011. . [6]"The Effect of Catalysts on Rates of Reaction." Chemguide: Helping You to Understand Chemistry - Main Menu. Web. 08 Oct. 2011. . [7]"Power Gains from a Sports Catalyst." Car Tuning & Modified Cars - How To... Guides. Web. 08 Oct. 2011. .
2. Cooper, M. M., Cooperative Chemistry Laboratory Manual, McGraw-Hill: New York, NY, 2009, p. 60.
middle of paper ... ... The Web. 22 Feb. 2014. http://www.chemheritage.org/discover/online-resources/chemistry-in-history>.
The purpose of the experiment is to study the rate of reaction through varying of concentrations of a catalyst or temperatures with a constant pH, and through the data obtained the rate law, constants, and activation energies can be experimentally determined. The rate law determines how the speed of a reaction occurs thus allowing the study of the overall mechanism formation in reactions. In the general form of the rate law it is A + B C or r=k[A]x[B]y. The rate of reaction can be affected by the concentration such as A and B in the previous equation, order of reactions, and the rate constant with each species in an overall chemical reaction. As a result, the rate law must be determined experimentally. In general, in a multi-step reac...
The reactions that take place to convert the harmful gasses to un-harmful gasses could not occur without the right amount of energy, for a reaction to take place it has to reach the correct activation energy. Activation energy is the minimum amount of energy that the reacting species must have in order to undergo the specified reaction. The catalytic converter helps the thermodynamic process by decreasing the activation energy needed for the reaction to take place. The catalyst will not form a product but will change the speed of the reaction.
If a reactant is a solid, then breaking it up into smaller pieces (but keeping the mass the same) will increase its surface area. If there is a larger surface area the reacting particles will have more of an area to react with, therefore there will be more collisions. 4. A catalyst works by giving the reacting particles something to stick to where they can collide with each other, because they are all attracted to the catalyst there are going to be more collisions. A catalyst does not get used up in a reaction.
Enzymes, are macromolecules which serve as catalysts. Catalysts are a chemical that can increase the rate of a chemical reaction or slow it down, without being changed by the reaction itself. The enzyme as a catalyst promotes the activity of the reactant which subsequently produces the product.
Living cells perform a multitude of chemical reactions very rapidly because of the participation of enzymes. Enzymes are biological catalysts, compounds that speed up a chemical reaction without being used up or altered in the reaction. The material with which the catalysts reacts, called the substrate, is modified during the reaction to form a new product. But because the enzyme itself emerges from the reaction unchanged and ready to bind with another substrate molecule, a small amount of enzyme can alter a relatively enormous amount of substrate.
being used up, for that is a property of a catalyst is, it speeds up a
There is an overwhelming use of catalysts - a substance that changes the rate of reaction without being consumed by the reaction itself- in various industrial processes. According to certain estimates [cite-wiki10] around 90% of all “commercially produced chemical products involve catalysts at some stage in the process of their manufacture.” Chemical products worth $900 billion were generated by catalytic processes worldwide in 2005 [cite – wiki11]. The close affiliation of the catalysts and the process of catalysis to a variety of industries and the proximity of these industries with consumers raise questions regarding the application of catalysts and their effects on products.
• The use of a catalyst will speed up the reaction as long as the catalysts electrode potentials are feasible for each step in the reaction. Since a catalyst lowers the activation energy and takes the reaction through a different route, according to the Maxwell-Boltzmann diagram, at a constant temperature more particles are able to react as demonstrated by the diagrams below:
There are five factors which affect the rate of a reaction, according to the collision theory of reacting particles: temperature, concentration (of solution), pressure (in gases), surface area (of solid reactants), and catalysts. I have chosen to investigate the effect of concentration on the rate of reaction. This is because it is the most practical way to investigate. Dealing with temperatures is a difficult task, especially when we have to keep constant high temperatures. Secondly, the rate equation and the constant k changes when the temperature of the reaction changes.
that the rate of reaction must be fast enough to make as much of the
Chemical kinetics is the study and examination of chemical reactions regarding re-arrangement of atoms, reaction rates, effect of various variables, and more. Chemical reaction rates, are the rates of change in amounts or concentrations of either products or reactants. Concentration of solutions, surface area, catalysts, temperature and the nature of reactants are all factors that can influence a rate of reaction. Increasing the concentration of a solution allows the rate of reaction to increase because highly concentrated solutions have more molecules and as a result the molecules collide faster. Surface area also affects a
One vital process in the human body observed in chemistry is the idea of chemical kinetics. Chemical kinetics is the study of the rate of reactions, or how fast reactions occur.1 Three factors that affect chemical kinetics are concentration, temperature, and catalysis. As the concentration of a substance increases, the rate of the reaction also increases.1 This relationship is valid because when more of a substance is added in a reaction, it increases the likelihood that the
To control the rates of chemical reactions is imperative to the continued existence of our species. Controlled chemical reactions allow us to move forward in society, constantly. We find new ways to provide light and heat our homes, cook our food, and pursue in crafts that benefit our society. There are, however, just as there are advantages, disadvantages to the efficiency of controlling the rate of reactions, which in some cases can be fatal to our scientific development and progression. The growth of humankind necessitates that we must be able to control the rate of chemical reactions.