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In the button cells widely used in watches and other devices the following reaction takes plance : Zn(s)+Ag_(2)O(s)+H_(2)O(l) rarr Zn^(2+)(aq)+2Ag(s)+2OH^(-)(aq) Determine Delta_(r )G^(@) and E^(@) for the reaction. |
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Answer» Solution :In the given cell, Zn is oxidised to `Zn^(2+)` and `Ag_(2)O` is REDUCED to Ag. `therefore E_("cell")^(@)=E_("cathode")^(@)-E_("ANODE")^(0)=[0.344-(-0.76)V]=1.104 V` `therefore Delta_(r )G^(@)=-nFE_("cell")^(@)=-2xx96500xx1.104=-2.13xx10^(5)J` |
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