Define (a) a coulomb, (b) an electric current, (c) an ampere, and (d) a faraday.
ID: 731380 • Letter: D
Question
Define (a) a coulomb, (b) an electric current, (c) an ampere, and (d) a faraday. Calculate the number of electrons that have a total charge of 1 coulomb. For each of the following cations, calculate (i) the number of faradays required to produce 1.00 mol of free metal and (ii) the number of coulombs required to produce 1.00 g of free metal, (a) Fe3+, (b) Sn2+, (c) Hg22+ For each of the following cations, calculate (i) the number of faradays required to produce 1.00 mol of free metal, and (ii) the number of coulombs required to produce 1.00 g of free metal. (a) Fe2+, (b) Au3+, (c) K+ In 400. min, 2.25 g of copper is obtained by electrolysis of a copper(I) acetate solution, (a) How many amperes is required for this experiment? (b) Using the same current and time, what mass of copper would be obtained from copper(II) nitrate solution? A mass of 1.20 g of silver is plated from a silver nitrate solution in 1.25 h. Calculate the (a) coulombs, (b) faradays and (c) amperes necessary tor this process.Explanation / Answer
(a) Fe+2
(i) No. of Faradays required to produce 1 mole of free metal
= 2 x 1.66 x 10^-24 F = 3.32 x 10^-24 F
(ii) No. of Columbs required to produce 1 gm of free metal
= (2 x 1.602 x 10^-19/55.845) C = 5.737 x 10^-21 C
(b) Au+3
(i) No. of Faradays required to produce 1 mole of free metal
= 3 x 1.66 x 10^-24 F = 4.98 x 10^-24 F
(ii) No. of Columbs required to produce 1 gm of free metal
= (3 x 1.602 x 10^-19/196.967) C = 2.44 x 10^-21 C
(c) K+
(i) No. of Faradays required to produce 1 mole of free metal
= 1.66 x 10^-24 F
(ii) No. of Columbs required to produce 1 gm of free metal
= (1.602 x 10^-19/39.098) C = 4.097 x 10^-21 C
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