Redox reaction
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Created on May 9, 2021
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Transcript
Application of Redox reaction
RedoxReaction
01
Combustion Reaction
02
03
04
05
Electro-ChemicalReaction
Photosynthesis Process
Extraction ofMetal
An oxidation-reduction (redox) reaction is a type of chemical reaction that involves a transfer of electrons between two species. An oxidation-reduction reaction is any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron.
A combustion reaction is a type of redox reaction that occurs when a substance combines with molecular oxygen to make oxygen-containing compounds of other elements in the reaction. One example is the burning of methane, the principal component of natural gas Oxygen (in its elemental form) is a crucial reactant in combustion reactions, and it is also present in the products. In combustion, the oxygen (O2) is reduced and the other elements are oxidized. Because of its abundance in the air, O2 is the most ubiquitous oxidizing agent on Earth.
Battery or petrochemical cells where the chemical energy is used to generate electricity is actually made of redox reaction principle. So we will have Cathode and Anode and they will be connected with a wire and bulb which can light up as electricity passes.
Redox reaction (oxidation-reduction reactions) are marked by the transfer of electrons. During oxidation, a substance tends to lose its electrons whereas, during reduction, a substance tends to gain electrons. Photosynthesis is a process in which chlorophyll convert the carbon dioxide into sugars in the presence of sunlight by a set of redox reactions. Calvin cycle represents a set of reactions which are used to remove electrons from water which are then used to turn carbon dioxide into organic compounds.
The redox reactions find a great deal of application in the extraction industry to extract metals or minerals from the natural ores. metals usually exist in an oxidized state in nature (due to their long term exposure to the oxygen present in the air surrounding them). hence, they need to be reduced in order to extract the required metal out of them. this is done in the industry on a large scale with the help of a suitable reducing agent, depending on the metal or ore which is to be refined. for example, iron is extracted from the oxidized ore of ferric oxide in a large blast furnace in the iron extracting and refining industries using coke as a reducing agent. the reaction takes of iron metal extraction from its oxidized natural ore takes place as follows: Here Fe2O3 reduced to Fe and C is oxidized to CO Alumina is extracted from aluminum oxide by passing an electric current through it. Here Al2O3 simultaneously reduced to Al and oxidized to O2