Application of electrolysis. Presentation "Strong and weak electrolytes" presentation of a lesson for an interactive whiteboard in chemistry (grade 9) on the topic Presentation on the topic of the use of electrolytes in medicine

"History of Medicine" - Craniotomy. Methods used in the study of the history of medicine. Sources of studying medicine of primitive society. Types of traditional medicine. Reliable coverage of the history of medicine. From the collection of T. Meyer-Steineg. Features of medicine of ancient civilizations. Types of ancient medicine. Ancient writing documents.

"Computers in medicine" - The master (driver) of the heart rate. Poll results. Examples of computer devices and methods of treatment and diagnostics. Respiratory and anesthesia devices. What and how did we learn about the use of computers in medicine? Computer technology used for learning medical workers practical skills. Based on the symptoms generated by the computer, the student must determine the course of treatment.

"Electrolysis of solutions and melts" - Chemistry. Cathode. Insoluble, simple, organic substances, oxides. Electrolytes are complex substances whose melts and solutions conduct electricity. CuSO4 + Fe = Cu + FeSO4. The process of donating electrons by ions is called oxidation. Avoid splashing electrolyte. Сu2+ is an oxidizing agent. Recovery (attachment e).

"Use of resources" - Psychological and pedagogical features of the formation and use of the catalog educational resources Internet networks. Directions for improving the Catalog 1. Enlargement of the list academic disciplines, further gradation into smaller subsections 2. Introduction of additional structuring criteria (for example, combining links to resources by type - simulators, games, etc.), 3. Increasing the number of links to methodological, technological and technical manuals 4. More detailed description teaching methods using educational resources.

"Laws of electrolysis" - Derivation of the formula. © Stolbov Yu.F., teacher of physics, secondary school №156 St. Petersburg 2007. The second law of electrolysis. Electrolytic dissociation is the breakdown of a substance into ions upon dissolution. Output. Electrolysis. m=kq. NaOH?Na++OH- HCl?H++Cl-CuSO4?Cu2++SO42-. Definitions. k=(1/F)X F=96500C/kg X=M/z. M-mass of matter q-transferred charge k-electrochemical equivalent.

"Application of electrolysis" - Application of electrolysis. Conductive. Obtaining chemically pure substances. Non-conductive. A copy of the bas-relief obtained by electroforming. 2. Electroplating. The electrochemical equivalent and the Faraday number are related by the relationship. Not containing free charged particles (non-dissociating). Electric current in liquids.




English physicist and chemist, one of the founders of electrochemistry At the end of the 18th century, he gained a reputation as a good chemist. In the early years of the 19th century, Davy became interested in studying the effect of electric current on various substances, including molten salts and alkalis.





To protect metals from oxidation, as well as to give products strength and better appearance they are covered thin layer noble metals (gold, silver) or low-oxidizing metals (chromium, nickel). The object to be electroplated is thoroughly cleaned, polished and degreased, after which it is immersed as a cathode in a galvanic bath. The electrolyte is a metal salt solution that is used for coating. The anode is a plate of the same metal. Electroplating Coating metals with a layer of another metal using electrolysis


To give the impression of electrical conductivity, it is covered with graphite dust, immersed in a bath as a cathode, and a layer of metal of the required thickness is obtained on it. Then, wax is removed by heating. To obtain copies from metal objects (coins, medals, bas-reliefs, etc.), casts are made from some plastic material(e.g. wax) Obtaining copies from objects using electrolysis Electroplating


Jacobi Boris Semenovich () - Russian physicist and inventor in the field of electrical engineering, developer of the electroforming process in the 19th century


Invented the first electric motor with direct rotation of the shaft Created a collector for rectifying the current Invented writing telegraph devices Moved the boat with the help of electrical energy Created devices for measuring electrical resistance, made a resistance standard, designed a voltmeter


Acid batteries The active substances of the battery are concentrated in the electrolyte and positive and negative electrodes, and the combination of these substances is called the electrochemical system. In lead-acid batteries, the electrolyte is a solution of sulfuric acid (H 2 SO 4), the active substance of the positive plates is lead dioxide (PbO 2), the negative plates are lead (Pb)










The relevance of electrolysis is explained by the fact that many substances are obtained in this way. organic matter(hydrogen, oxygen, chlorine, alkalis, etc.) Production of metals (lithium, sodium, potassium, beryllium, magnesium, zinc, aluminum, copper, etc.) Purification of metals (copper, silver,…) Production of metal alloys Obtaining galvanic coatings Treatment of metal surfaces (nitriding, boriding, electropolishing, cleaning) Obtaining organic substances Electrodialysis and water desalination Film deposition using electrophoresis


Links to sources of information and images: I.I. Novoshinsky, N.S. Novoshinsky Chemistry profile level 10 class Primenenie-elektroliza.jpg G. Ya. Myakishev, B. B. Bukhovtsev N. N. Sotsky Physics Grade 10

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The essence of electrolysis Electrolysis is a redox
the process that occurs on the electrodes during the passage
direct electric current through the solution or
electrolyte melt.
To carry out electrolysis to the negative
pole of an external DC source
connect the cathode, and to the positive pole -
anode, after which they are immersed in an electrolyzer with
electrolyte solution or melt.
The electrodes are usually metal, but
non-metallic ones, such as graphite, are also used
(conducting current).

As a result of electrolysis on the electrodes (cathode and
anode) the corresponding products are released
reduction and oxidation, which, depending on
conditions can react with
solvent, electrode material, etc., - so
called secondary processes.
Metal anodes can be: a)
insoluble or inert (Pt, Au, Ir, graphite
or coal, etc.), during electrolysis they serve only
electron transmitters; b) soluble
(active); during electrolysis, they are oxidized.

In solutions and melts of various electrolytes
there are ions of opposite sign, i.e. cations and
anions that are in random motion.
But if in such an electrolyte melt, for example
melt sodium chloride NaCl, lower the electrodes and
pass a direct electric current, then the cations
Na+ will move towards the cathode, and Cl– anions will move towards the anode.
The process takes place at the cathode of the electrolyzer
reduction of Na+ cations by electrons of external
current source:
Na+ + e– = Na0

At the anode, the process of oxidation of chlorine anions takes place,
moreover, detachment of excess electrons from Cl–
is carried out due to the energy of an external source
current:
Cl– – e– = Cl0
Emitted electrically neutral chlorine atoms
join together to form a molecular
chlorine: Cl + Cl = Cl2, which is released at the anode.
The overall equation for the electrolysis of a chloride melt
sodium:
2NaCl -> 2Na+ + 2Cl– -electrolysis-> 2Na0 +
Cl20

Redox action
electric current can be many times
stronger than the action of chemical oxidants and
reducing agents. Changing the voltage to
electrodes, you can create almost any force
oxidizing agents and reducing agents that
are the electrodes of the electrolytic bath
or electrolyzer.

It is known that none of the strongest chemical
an oxidizing agent cannot take away F– from the fluoride ion
electron. But this is feasible with electrolysis,
e.g. molten NaF salt. In this case, the cathode
(reductant) is released from the ionic state
metallic sodium or calcium:
Na+ + e– = Na0
on the anode (oxidizing agent), a fluorine ion F– is released,
going from a negative ion to a free ion
condition:
F– – e– = F0 ;
F0 + F0 = F2

Products released on the electrodes
can enter into chemical
interaction, therefore anodic and cathodic
the space is separated by a diaphragm.

Practical application of electrolysis

Electrochemical processes are widely used in
various areas of modern technology, in
analytical chemistry, biochemistry, etc. In
chemical industry electrolysis
receive chlorine and fluorine, alkalis, chlorates and
perchlorates, persulfuric acid and persulfates,
chemically pure hydrogen and oxygen, etc. When
in this case, some substances are obtained by reduction
on the cathode (aldehydes, para-aminophenol, etc.), others
electrooxidation at the anode (chlorates, perchlorates,
potassium permanganate, etc.).

Electrolysis in hydrometallurgy is one of the
processing stages of metal-containing raw materials,
ensuring the production of commodity metals.
Electrolysis can be carried out with soluble
anodes - electrorefining process or with
insoluble - the process of electroextraction.
The main task in the electrorefining of metals
is to ensure the necessary purity of the cathode
metal at acceptable energy costs.

In non-ferrous metallurgy, electrolysis is used to
extraction of metals from ores and their purification.
Electrolysis of molten media is obtained
aluminum, magnesium, titanium, zirconium, uranium, beryllium and
others
For refining (cleaning) metal
plates are cast from it by electrolysis and placed
them as anodes in the electrolyzer. When passing
current, the metal to be cleaned is subjected to
anodic dissolution, i.e. goes into solution in the form
cations. These metal cations are then discharged into
cathode, resulting in the formation of a compact deposit
already pure metal. Impurities in the anode
either remain insoluble or go into
electrolyte and removed.

Electroplating - applied area
electrochemistry dealing with processes
applying metal coatings to
surface of both metal and
non-metal products when passing
direct electric current through
solutions of their salts. Electroplating
subdivided into electroplating and
electroplating.

Electroplating (from Greek to cover) is electrodeposition on
metal surface of another metal that is firmly
binds (adheres) to the coated metal (object),
serving as the cathode of the electrolyzer.
Before coating the product, its surface must be
thoroughly clean (degrease and pickle), otherwise
case, the metal will be deposited unevenly, and in addition,
adhesion (bond) of the coating metal to the surface of the product
will be unstable. By electroplating, you can cover
detail with a thin layer of gold or silver, chrome or nickel. FROM
using electrolysis, you can apply the thinnest
metal coatings on various metal
surfaces. With this coating method, the part
used as a cathode placed in a salt solution of that
metal to be coated. As
the anode is a plate of the same metal.

Electroplating - obtaining by electrolysis
precise, easily detachable metal copies
relatively significant thickness with different
non-metallic and metallic objects,
called matrices.
Busts are made using electroforming,
statues, etc.
Electroplating is used to apply
relatively thick metal coatings on
other metals (for example, the formation of a "consignment note"
layer of nickel, silver, gold, etc.).

 

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