Consider an electrochemical cell involving the overall reaction... Consider an e

Question

Consider an electrochemical cell involving the overall reaction...

Consider an electrochemical cell involving the overall reaction 2AgBr(s) + Pb(s) rightarrow Pb^2+(aq) + 2Ag(s) + 2 Br^- (aq) Each half-reaction is carried out in a separate compartment. The anion included in the lead half-cell is NO3^- The cation in the silver half-cell is K^+. The two half-cells are connected by a KNO3 salt bridge. If [Pb^2+] = 1.0 M and [Br^-] = 0.14 M, what is the emf of the cell at 298 K? Given: AgBr(s) + e^- rightarrow Ag(s) + Br^- (aq) Edegree = +0.07 V. Pb^+2 + 2e^- rightarrow Pb(s) Edegree = - 0.13 V.

Explanation / Answer

nernst equation E = Eo - 0.0591/n log Q

E = 0.2 - (0.0591/2) (log [1][0.14]2)

E = 0.25 V

so answer option C

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---