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Aplications of the oxidation-reduction process
Galvanic cells, also known as voltaic cells, are devices that generate electric current from a spontaneous oxidation-reduction chemical reaction, supplying electrical current through the transfer of electrons.
Megnyitás
Aplications of the oxidation-reduction process Applications of electrochemical reactions Industry Molten NaCl electrolysis: method widely used in industry to obtain sodium and chlorine in its elemental state Mettalic coatings, electroplating: applying a thin layer of metal on an electronic current conducting surface Electric batteries: They are the industrialized and commercial formats of galvanic cells. (car batteries are the traditional battery model) Nature Corrosion in metals Electric eels Nerve impulses generated neurons Electrolytic cells To force a chemical reaction that would otherwise not occur Electrochemical cell in which electrical energy is used to drive a non-spontaneous oxidation-reduction reaction Galvanic or voltaic cells Function To supply electrical current through a redox reaction to the transfer of electrons Definition Devices capable of generating an electric current from a spontaneous chemical reaction of oxidation-reduction Steps to balance a redox reaction Check that both sides of the equation have the same number of atoms of each element Balance the remaining elements that do not oxidize or reduce to obtain the balanced equation Transfer the coefficient that appears in front of each substance in the half-balanced reactions Match the number of electrons lost in oxidation to the number of electrons gained in reduction Balance the charge in each equation. This should be done after the balance of mass. Perform the balance of mass. Same number of chemical species on both sides Write the two oxidation and reduction half-reactions Identify the elements that change their oxidation state or charge Assign the oxidation numbers to each element in the reaction Oxidation number Are the assigned charges to the different atoms involved of a species Oxidizing and reducing agents Reducing agent Increases its oxidation number Loses electrons Oxidizing agent Decreases its oxidation number Gain electrons Oxidation and reduction concepts Reduction: electron gain Oxidation: loss of electrons Whenever one species is reduced, there is another that is oxidized
