Silver tarnish is the result of the oxide on the silver surface reacting with hydrogen sulfide (H2S) in air. This leaves a black film of silver sulfide (Ag2S).Polishing the tarnished silver will restore the shine but at the expense of some of the silver metal. An alternative process is to allow aluminumto reduce the silver in the presence of a solution of sodium bicarbonate (baking sodium) electrolyte. 1. Assume that Aluminumand Silver Sulfideare the starting substances (reactants) in the reaction: a.Write a balanced chemical equation describing the ”re-creation” of silver, using the information in the case study.    b.State the names of the products that are produced from this reaction.   c.What type of reaction(s) is/are being represented by the chemical reaction you wrote in part (a)?   d.Is the reaction in part (a) an oxidation-reduction (redox) reaction?     e.If this is a redox reaction, then identify the following:   What is undergoing oxidation (what is being oxidized)? Support your answer using oxidation numbers.   What is undergoing reduction (what is being reduced)? Support your answer using oxidation numbers.   What is the reducing agent?   What is the oxidizing agent?

Q: tatement is true. Remember that any spontaneously operating cell has a positive cell value. Aluminum…

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Q: An aqueous solution of AICI3 is electrolyzed for 1.50 hours producing 5.45 g of aluminum What is the…

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Q: Aluminum requires relatively little protection from corrosion because.....   aluminum has little…

A: Aluminum is a reactive metal .It easily  get oxidized in the presence of oxygen .

Q: In a particular redox reaction, SO3 is oxidized to SO2 and Ag+ is reduced to Ag. Complete and…

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Q: What is the oxidation number of Fe in: FeOOH Fe2O3 Fe3O4

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Q: Complete and balance the following half-reaction in acidic solution. TiO2(s) ---> Ti2+(aq)

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Q: Which one of these metals reacts with an acid to produce hydrogen gas? Hg, Cr, or Pt?

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Q: a student carries out this chemical reaction in a beaker  Zn+CuCl2 -> Cu+ZnCl2 after the reaction…

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Q: When solid Fe metal is put into an aqueous solution of NiSO4, solid Ni metal and a solution of FeSO4…

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Q: The oxidation number of platinum in Pt(H2O)4 ^+2 is

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Q: What are the oxidation numbers of aluminum in Al(s) and Al2O3

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Q: a Nitrogen(II) oxide and hydrogen gases react to form ammonia gas and steam. b Hydrogen peroxide…

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Q: ) Metal Plating is a common process. What is it? How is it done? Give a basic description of the…

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.