electrochemistry

Question: For the cell reaction $2Hg(l)+2A{{g}^{+}}(aq)\to 2Ag(s)+Hg_{2}^{2+}(aq)$ It is the given that $E_{A{{g}^{+}}/Ag}^{0}=0.800V,\,[A{{g}^{+}}]={{10}^{-3}}M$ $E_{Hg_{2}^{2+}/Hg}^{0}=0.785V$ and $[Hg_{2}^{2+}]={{10}^{-1}}M$

1) The forward reaction is spontaneous

2) The backward reaction is spontaneous

3) ${{E}_{\text{cell}}}=1.585\,V$

4) ${{E}_{\text{cell}}}=3.170\,V$

Solution:

Explanation: No Explanation

Electrode potential Ecell Nernst equation and ECS

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