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Two half cell reactions of an electrochemical cell are given below : `MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-),toMn^(2+)(aq)+4H_(2)O(l),E^(@)=+1.51V` `Sn^(2+)(aq)toSn^(4+)(aq)+2e^(-),E^(@)=+0.51V` Construct the redox equation from the two half cell reactions and predict if theis reaction favours formation of reaction or product shown in the equation. |
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Answer» over all redox equation is `5Sn^(2+)(aq)+2MnO_(4)^(-)(aq)+16H^(+)(aq)to5Sn^(4+)(aq)+2Mn^(2+)(aq)+8H_(2)O(l)` `E_(cell)^(@)=E_("cathode")^(@)-E_("anode")^(@)=1.51-(-0.15)=+1.66V` The reaction favours formation of products. |
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