Categories > electrochemistry > Electrode potential > The standard reduction potential ${{E}^{0}}$ for the half reactions are as $Zn=Z{{n}^{2+}}+2{{e}^{-}};\,{{E}^{0}}=+0.76\,V$; $Fe=F{{e}^{2+}}+2{{e}^{-}};\,{{E}^{0}}=+0.41\,V$; The emf for cell reaction $F{{e}^{2+}}+Zn\to Z{{n}^{2+}}+Fe$ is

electrochemistry

Question: The standard reduction potential ${{E}^{0}}$ for the half reactions are as $Zn=Z{{n}^{2+}}+2{{e}^{-}};\,{{E}^{0}}=+0.76\,V$; $Fe=F{{e}^{2+}}+2{{e}^{-}};\,{{E}^{0}}=+0.41\,V$; The emf for cell reaction $F{{e}^{2+}}+Zn\to Z{{n}^{2+}}+Fe$ is


1) – 0.35 V
2) + 0.35 V
3) + 1.17 V
4) – 1.17 V
Solution: Explanation: No Explanation
Electrode potential Ecell Nernst equation and ECS

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