Suppose 250.mL of a 0.455 M solution of CuCl2 is electrolyzed. How long will a c

Question

Suppose 250.mL of a 0.455 M solution of CuCl2 is electrolyzed. How long will a current of 0.750A have to run in order to reduce the concentration of Cu2+ to 0.167 M? what mass of Cu(s) will be deposited on the cathode during this time? Three electrolytic cells arc connected in series; the currant passes through all throe, ore after another. In the first cell. 1.20 g of Cd is oxidized to Cd2+; in the second, Ag+ is reduced to Ag, in the third. Fe2+ is oxidized to Fe3+ . I in the number of faradays passed through the circuit. What mass of Ag is deposited at the cathode in the second ceil? What mass of Fc(NO3) might be recovered from the third cell solution? Which is the stronger oxidizing agent? Zn2+ or Ca2+ Cr3+ or Cu2+

Explanation / Answer

sol: suppose that, so we get, M(Ag) = 107,87 g/mole n(Ag) = m(Ag) / M(Ag) n(Ag) = 0,634•10^-3/107,87 n(Ag) = 5,877•10^-6 mole . . . according to the equation : n(e(-)) = n(Ag) = 5,877•10^-6 mole 1 mole of e(-) ----------------> F= 96 485,3415 C 5,877•10^-6 mole of e(-) ----------------> Q = F x 5,877•10^-6 = 0,567 C answer . .

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