example decomposition chemical reaction
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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.
The generalized reaction for chemical decomposition is:
- AB → A + B
- 2H2O(I) → 2H2 + O2
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
- MCO3→ MO + CO2
A specific example of this involving calcium carbonate:
- CaCO3→ CaO + CO2
- 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, 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
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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
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.
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).
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.]