electrochemistry

Question: The standard oxidation potential of zinc and silver in water at $298 K$ are $Zn\,(s)\to Z{{n}^{2+}}+2{{e}^{-}};\,E=0.76\,V$ $Ag\,(s)\to A{{g}^{+}}+{{e}^{-}};\,E=-0.80\,V$ Which of the following reactions actually take place

1) $Zn\,(s)+2A{{g}^{+}}(aq)\to Z{{n}^{++}}(aq)+2Ag\,(s)$

2) $Z{{n}^{++}}(aq)+2Ag\,(s)\to 2A{{g}^{+}}(aq)+Zn\,(s)$

3) $Zn\,(s)+Ag\,(s)\to Z{{n}^{++}}(aq)+A{{g}^{+}}(aq)$

4) $Z{{n}^{++}}(aq)+A{{g}^{+}}\,(s)\to Zn\,(s)+Ag\,(s)$

Solution:

Explanation: No Explanation

Electrode potential Ecell Nernst equation and ECS

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