A voltaic cell consists of an Mn/Mn 2+ half-cell and aPb/Pb 2+ half-cell. Calcul
ID: 681399 • Letter: A
Question
A voltaic cell consists of an Mn/Mn2+ half-cell and aPb/Pb2+ half-cell. Calculate [Pb2+] when[Mn2+] is 2.5 M andEcell = 0.51 V.Explanation / Answer
E0 Pb2+/Pb = -0.13 E0 Mn2+/Mn = -1.18 => since E0 Pb2+/Pb is more , so Pb2+ will get reduced and Mnwill be oxidized => reactions taking place are:: Mn------------> Mn2+ +2e- 1.18 Pb2+ + 2e- ------>Pb -0.13 -------------------- Mn+ Pb2+ ---------> Pb + Mn2+ E0cell = 1.18-0.13 =1.05V since Ecell = E0cell -(0.0591/n)Log[K] K= [Mn2+]/[Pb2+] and n=2 ( 2 electrons involved), Mn2+ = 2.5 so Ecell = 1.05-(0.0591/2)log(2.5/[Pb2+]) = 0.51 (given) => Pb2+ = 1.329 x 10^-18
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