Given that standard electrode potentials`(E^(@))` of metals are :
`K^(+)//K=-2.93" V",Ag^(+)//Ag=0.80" V",Cu^(2+)//Cu=0.34" V", Mg^(2+)//Mg=-2.37" V"`
`Sn^(2+)(aq) to Sn^(4+)(aq)+2e^(-),E^(@)=-0.15" V"`
Construct the redox reaction equation from the two half-reactions and calculate the cell potential from the standard potentials and predict if the reaction is reactant or product favoured.

Explanation

Please note that less the `E^(@)` value of an electrode, more is its reducing power. The increasing order of reducing power is :
`Ag^(+)//Ag lt Cu^(2+)//Cu lt Fe^(2+)//Fe lt Mg^(2+)//Mg lt K^(+) lt K`.