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.

Explanation

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.