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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>.
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.
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.
Therefore, it can be concluded that a catalyst has a major effect upon the time taken in a reversible reaction to reach equilibrium in a closed system, but does not have any effect the macroscopic properties of the system.
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.
being used up, for that is a property of a catalyst is, it speeds up a
...ctions that have very low activation energies, this means that they happen very quickly or almost instantaneously. On the other hand, there are multitudes of reactions that have exceptionally high activation temperatures and these reactions take much longer to take place. With this in mind, it is important to remember that not all collisions create a reaction. Millions of molecules collide with each other every second, but not all of them react. The molecules must have reached an appropriate kinetic energy to break the bonds of reactants to create products. “When two billiard balls collide, they simply bounce off of each other… In order to… initiate a reaction, collisions must be sufficiently energetic (kinetic energy) to bring about this bond disruption.” (boundless.com). The bonds of reactions can only be broken when molecules of certain kinetic energies collide.
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.
The aim of this experiment was to investigate the affect of the use of a catalyst and temperature on the rate of reaction while keeping all the other factors that affect the reaction rate constant.
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.
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
that the rate of reaction must be fast enough to make as much of the
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.
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.