`CuSO_4 (aq) + Fe (s) to FeSO_4 (aq) + Cu (s)`
Divide the above equation into oxidation and reduction half reactions.

Divide the following redox reactions into oxidation and reduction half reactions. Zn + Cu^(2+) to Zn&(2+) + Cu

CuSO_(4)(aq.)+Zn(s) to ZnSO_(4)+Cu darr

CuSO_(4)(aq.)+Zn(s) to ZnSO_(4)+Cu uarr

CuSO_(4)+Zn(s) to ZnSO_(4)+Cu

Write the equation in the ionic form CuSO_4 (aq) + Fe (s) to FeSO_4 (aq) + Cu (s)

(CU^(+) ((aq)) is unstable in solution and undergoes simultaneous oxidation and reduction, according to the reaction 2Cu_((aq))^(+) Cu_((aq))^(2+) +Cu_((s)) choose E^(@) for the above reaction if E_(Cu^(2+)//Cu^(@))= 0.34V and E_(Cu^(2+)//Cu^(+) )= 0.15V

Cu^(2+)(aq.) is unstable in solution and under goes simultaneous oxidation and reduction according to the reaction 2Cu^(+)(aq.)hArr Cu^(2+)(aq.)+Cu(s) Choose the correct E^(@) for the above reaction if E_(Cu^(2+))^(@)//Cu = 0.34 V and E_(Cu^(2+))^(@)//Cu^(+) = 0.15 V

Zn(s) + Cu^(2+)(aq) rarr Zn^(2+)(aq) + Cu(s) The cell representation for the above redox reaction is

FeSO_(4)+Na_(2)S to FeS darr

Standard reduction potential of the half cell reactions are given below Co^(3+)(aq) + e^(1-) to Co^(2+)(aq) , E^0 = +1.81 V Au^(3+)(aq) + 3e^(1-) to Au(s) , E^0 = +1.40 V I_(2)(s) + 2e^(1-) to 2I^(-)(aq) , E^0 = +0.54 V Cu^(2+)(aq) + 2e^(1-) to Cu(s) , E^0 = +0.34 V The strongest oxidizing and reducing agents respectively are: