Categories > electrochemistry > Electrode potential > $Z{{n}^{2+}}+2{{e}^{-}}\to Zn(s);\,{{E}^{0}}=-0.76$; $F{{e}^{3+}}+{{e}^{-}}\to F{{e}^{2+}};\,{{E}^{0}}=-0.77$; $C{{r}^{3+}}+3{{e}^{-}}\to Cr;\,{{E}^{0}}=-0.79$; ${{H}^{+}}+2{{e}^{-}}\to 1/2{{H}_{2}};\,{{E}^{0}}=0.00$; Strongest reducing agent is

electrochemistry

Question: $Z{{n}^{2+}}+2{{e}^{-}}\to Zn(s);\,{{E}^{0}}=-0.76$; $F{{e}^{3+}}+{{e}^{-}}\to F{{e}^{2+}};\,{{E}^{0}}=-0.77$; $C{{r}^{3+}}+3{{e}^{-}}\to Cr;\,{{E}^{0}}=-0.79$; ${{H}^{+}}+2{{e}^{-}}\to 1/2{{H}_{2}};\,{{E}^{0}}=0.00$; Strongest reducing agent is


1) $F{{e}^{2+}}$
2) $Zn$
3) $Cr$
4) ${{H}_{2}}$
Solution: Explanation: No Explanation
Electrode potential Ecell Nernst equation and ECS

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