electrochemistry

Question: For the electrochemical cell, $M|{{M}^{+}}||{{X}^{-}}|X,\,{{E}^{0}}({{M}^{+}}/M)=0.44\,V$ and ${{E}^{0}}(X/{{X}^{-}})=0.33\,V$. From this data one can deduce that

1) $M+X\to {{M}^{+}}+{{X}^{-}}$ is the spontaneous reaction

2) ${{M}^{+}}+{{X}^{-}}\to M+X$ is the spontaneous reaction

3) ${{E}_{\text{cell}}}=0.77\,V$

4) ${{E}_{\text{cell}}}=-0.77\,V$

Solution:

Explanation: No Explanation

Electrode potential Ecell Nernst equation and ECS

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