Calculate the E for a cell with the overall redox reaction given below and an in

Question

Calculate the E for a cell with the overall redox reaction given below and an initial concentration of Mg^2+ equal to 0.5 M and a concentration of Sn^2+ equal to 0.010 M. Mg (s) + Sn^2+ rightarrow Sn (s) + Mg^2+ E^0 = 2.59 Temperature = 298.15 a) 2.54 V b) 2.64 V c) 2.65 V d) none of the above What is the E for the reaction given below at a pH of 6.83 if the initial concentration other reactant and product species is 0.1 M? Temperature = 298.15 K MnO_4^- (aq) + 2H^+ + Bi (s) rightarrow BiO^+ (aq) + MnO_2 (s) + H_2 O (l) E^0 = 1.36 V.

Explanation / Answer

Q9

Apply Nernst equation for non standard conditions

E = Eº -0.0592/n*log(Q)

Recall that Q = product/reactant coefficient

n = 2 electrons are being transferred

Q = (Mg+2)/(Sn+2) = 0.5/0.01 = 50

E = 2.59 - 0.0592/2 * log(50)

E = 2.53971

E = 2.54 V

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