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From Wikipedia

Chemical decomposition

Chemical decomposition, analysis or breakdown is the separation of a chemical compound into elements or simpler compounds. It is sometimes defined as the exact opposite of a chemical synthesis. Chemical decomposition is often an undesired chemical reaction. The stability that a chemical compound ordinarily has is eventually limited when exposed to extreme environmental conditions like heat, radiation, humidity or the acidity of a solvent. The details of decomposition processes are generally not well defined, as a molecule may break up into a host of smaller fragments. Chemical decomposition is exploited in several analytical techniques, notably mass spectrometry, traditional gravimetric analysis, and thermogravimetric analysis.

A broader definition of the term decomposition also includes the breakdown of one phase into two or more phases.

There are broadly three types of decomposition reactions: thermal, electrolytic and catalytic.

Reaction formula

The generalized reaction for chemical decomposition is:

AB → A + B

with a specific example being the electrolysis of water to gaseous hydrogen and oxygen:

2H2O(I) → 2H2 + O2

Additional examples

An example of spontaneous decomposition is that of hydrogen peroxide, which will slowly decompose into water and oxygen:

2H2O2→ 2H2O + O2

Carbonates will decompose when heated, a notable exception being that of carbonic acid, H2CO3. Carbonic acid, the "fizz" in sodas, pop cans and other carbonated beverages, will decompose over time (spontaneously) into carbon dioxide and water

H2CO3→ H2O + CO2

Other carbonates will decompose when heated producing the corresponding metaloxide and carbon dioxide. In the following equation M represents a metal:

MCO3→ MO + CO2

A specific example of this involving calcium carbonate:

CaCO3→ CaO + CO2

Metal chlorates also decompose when heated. A metal chloride and oxygen gas are the products.

2MClO3→ 2MCl + 3O2

A common decomposition of a chlorate to evolve oxygen utilizes potassium chlorate as follows:

2KClO3→ 2KCl + 3O2

Many metal carbonates decompose to form metal oxides and carbon dioxide when heated.

Chemical decomposition

Chemical decomposition, analysis or breakdown is the separation of a chemical compound into elements or simpler compounds. It is sometimes defined as the exact opposite of a chemical synthesis. Chemical decomposition is often an undesired chemical reaction. The stability that a chemical

From Yahoo Answers

Question:can you please give me examples of these chemical reactions 1. Synthesis 2. Decomposition 3. Single Displacement 4. Double Displacement

Answers:1. 2 H2(g) + O2(g)--->2 H2O,(l) synthesis 2 .2 H2O-(l)--> O2)g)+2 H2 (g) , decomposition 3. 2NaCl(aq)+ F2(g)--->2 NaF(aq)+ Cl2(g), single displacement 4. AgNO3(aq)+ NaCl(aq)---> AgCl(s) + NaNO3(aq), double displacement

Question:The following is an example of reactions involving heterogeneous catalysts: the decomposition og phosphine (PH3) over tungsten (W) (a solid catalyst): 4PH3(g) -> P4(g) + 6H2(g) The rate of the above reaction is found to be independent of the pressure of PH3 as long as the pressure of PH3 is sufficiently high (say >= 1 atm). Explain.

Answers:Lancenigo di Villorba (TV), Italy LET ME RECOVER THE EXPERIMENTAL FACTs, HENCE I SHOW MY REASONINGs. EXPERIMENTAL FACTs Phosphine undergoes decomposition in Its Chemical Elements if it flows upon a TUNGSTEN-BASED powder which is able to acts as a CATALYST : meanwhile TUNGSTEN maintain its chemical nature, it enhances the Decomposition's Rate which runs VERY FASTER THAN when Catalyst there wasn't. If the Partial Pressure of Phosphine results GREATER THAN a THRESHOLD VALUE, Kinetic Data show a Decomposition's Rate iniflunced by Partial Pressure. DISCUSSION The mechanism related to this Decomposition experiment involves FIVE MAIN STEPs, as the following ones : -) Phosphine must diffuse from Gas Bulk toward the TUNGSTEN's surface ; -) Phosphine interact with Tungsten's surface, e.g. Tungsten ADSORBs Phosphine ; -) Adsorbed Phosphine forms Secundary Chemical Bonds with Tungsten, so the Decomposition take place giving Phosphorus Atoms and Hydrogen Ones in the BOUND FORM TO TUNGSTEN ; -) Phosphorus and Hydrogen's BOUND FORMs break its Chemical Bonds ; -) Phosphorus and Hydrogen diffuse outward. RATE DETERMINING STEP's approach assumes that the Decomposition's Rate results EQUAL THAN the Lowest's One among Its Five Elementar Step's Rates. In particular way, ii) STEP is related to ISOTHERMAL BEHAVIOUR of ADSORPTION, e.g. it states that it exists a THRESHOLD VALUE of Gas Molarity leading the Adsorption Equilibria to Its Maximum's Values. I hope this helps you.

Question:In my Grade 10 Science course, there is a question that I have to base a whole project around or I don't get my credit. The question is: "Research and list an example from everyday life for each of the five types of chemical reactions." the 5 types of chemical reactions are (if I remember correctly) Synthesis, Decomposition, Combustion, Single Displacement, Double Displacement. I need an example of each of those types of reactions that relate to everyday life. I think that NaCl (table salt) is a Synthesis because it's Na Cl -> NaCl right? But I need some examples from everyday life for all the others please. Thanks in advance.

Answers:Your 10th grade chemistry class probably won't really give you the correct names of all the reaction types, but those are basically it. There are also lots more reaction types, but you won't cover those until later. Your 10th grade chemistry class will be filled with half-truths and broad horrible generalizations, but at least you will be exposed to chemistry. Na^+ + Cl^- --> NaCl is true, and would fall under synthesis reactions. A (formerly?) common decomposition reaction would be sodium bicarbonate's reaction that puts out fires (in fire extinguishers): 2NaHCO3 --> Na2CO3 + H2O + CO2. It is effective at putting out fires because of the CO2 blocking Oxygen getting to the fire, the H2O absorbing some of the heat, and then there is the fact that the reaction itself is endothermic, or that when it happens the area around gets a little colder. Combustion is a very common reaction - it's what makes our cars go, and it's what burning is. Basically it's something containing carbon reacts with oxygen to form CO2 and H2O. Here's a simple example of the combustion of Methane, a common "natural gas": CH4 + 2O2 --> CO2 + 2H2O There's no such "Single Displacement reaction" in my vocabulary. The closes thing I can think of would be an aqueous redox reaction: Mg + 2AgNO3 (silver nitrate) --> Mg(NO3)2 (magnesium nitrate) + 2Ag A "double displacement reaction" is actually called a metathesis reaction. It is a common reaction in aqueous salts: NaCl + AgNO3 --> NaNO3 + AgCl (this one is cool because AgCl is insoluble, so it's like putting two liquids together and getting a solid out of it).

Question:Science Homework... My homework asks for 3 types of reactions that are important to life. Then my teacher wants me to describe reaction and show how it's important to life. So the only types of chemical reactions I know are synthesis reaction, decomposition reaction, single-displacement reaction, and double-replacement reaction. I know what they do, but the only reactions I find useful for everyday life are synthesis reaction and decomposition reaction. How are single-replacement reaction and double-replacement reactions important to everyday life? O yea, what breaks down into glucose? Is it sucrose or just food? Thanks!

Answers:I would suggest: Photosynthesis reaction is a good start Chlorophyll +CO2 makes O2 Then the other one Hemoglobin exchanging CO2 against O2 and the other way around. in the lungs O2 binds is then transported to the cells where it is used and replaced by CO2. Both these are Lewis acid base reactions. The last one I would suggest is a basic oxidation CH4+ 2O2 -> 2H2O + CO2 + energy This is important to everyday life as this is the basis for heating our houses. Ion reactions are important for your body too as you have a finely tuned balance if ions inside and outside your cells, but I haven't got a good example handy. [Ah, lastly the starch in your food is made into glucose.]

From Youtube

Chemistry - Synthesis, Decomposition and Combustion Reactions :GET the PowerPoint at www.ZUMAed.com. After a review of chemical reactions, this module presents a discussion of the characteristics of synthesis, decomposition, and combustion reactions, including examples of each. 3 By the end of this presentation, students will be able to * Describe what happens during a chemical reaction. * Identify signs that a chemical reaction has occurred. * Describe what happens during a synthesis, decomposition, and combustion reaction. * Identify and describe examples of synthesis, decomposition, and combustion reactions.

Decomposition Reaction Example :This is a short explaination, along with an example, of a decomposition reaction for my 9th grade chemistry project.