23.03.2023 - 09:52

Silver-plated tableware is prepared by electrochemically depositing Ag over the surface of a utensil fabricated from a less expensive material. Determine whether or not it would be possible to silver-

Question:

Silver-plated tableware is prepared by electrochemically depositing Ag over the surface of a utensil fabricated from a less expensive material. Determine whether or not it would be possible to silver-plate an Fe fork by suspending the fork in 1M AgNO3 solution. Briefly explain, including an equation for the reaction and a calculation of the net EMF.

Answers (1)
  • Estelle
    April 9, 2023 в 13:14
    It is possible to silver-plate an Fe fork by suspending the fork in 1M AgNO3 solution. The electrochemical reaction that occurs is as follows: Fe(s) + 2Ag+(aq) ? Fe2+(aq) + 2Ag(s) The iron atoms on the surface of the fork are oxidized to Fe2+ ions, while Ag+ ions in the solution are reduced to form a thin layer of silver metal on the surface of the fork. This process occurs due to the difference in the reduction potentials between Fe and Ag. The net EMF of the reaction can be calculated using the Nernst equation: EMF = E° - (RT/nF) * ln(Q) Where E° is the standard reduction potential, R is the gas constant, T is the temperature in Kelvin, n is the number of electrons transferred in the reaction, F is Faraday's constant, and Q is the reaction quotient. For the given reaction, the standard reduction potentials are: Fe2+(aq) + 2e- ? Fe(s) E° = -0.44 V Ag+(aq) + e- ? Ag(s) E° = 0.80 V The net EMF of the reaction is therefore: EMF = 0.80 V - (-0.44 V) = 1.24 V This indicates that the reaction is spontaneous and the silver plating process will proceed until all the available Ag+ ions in the solution are consumed.
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