Calculate the standard electrode potential for the following redox reaction in acidic medium using the standard reduction potentials given below:Fe²⁺(aq) + MnO₄^-(aq) + H⁺(aq) → Fe³⁺(aq) + Mn²⁺(aq) + H₂O(l)Standard reduction potentials:Fe³⁺(aq) + e^- → Fe²⁺(aq) E_o = +0.77 VMnO₄^-(aq) + 8H⁺(aq) + 5e^- → Mn²⁺(aq) + 4H₂O(l) E_o = +1.51 V

Question

Calculate the standard electrode potential for the following redox reaction in acidic medium using the standard reduction potentials given below:Fe²⁺(aq) + MnO₄^-(aq) + H⁺(aq) → Fe³⁺(aq) + Mn²⁺(aq) + H₂O(l)Standard reduction potentials:Fe³⁺(aq) + e^- → Fe²⁺(a

Answer 1

To calculate the standard electrode potential for the given redox reaction, we first need to balance the redox reaction and then use the Nernst equation.Balancing the redox reaction:1. Balance the atoms other than H and O:Fe  Fe + e  1 MnO + 5e  Mn  2 2. Balance the oxygen atoms by adding HO:Fe  Fe + e  1 MnO + 5e  Mn + 4HO  2 3. Balance the hydrogen atoms by adding H:Fe  Fe + e  1 MnO + 8H + 5e  Mn + 4HO  2 4. Balance the charges by multiplying the half-reactions by appropriate factors:5 Fe  Fe + e   1 1 MnO + 8H + 5e  Mn + 4HO   2 5. Add the half-reactions:5Fe + MnO + 8H  5Fe + Mn + 4HONow, we can use the Nernst equation to calculate the standard electrode potential for the balanced redox reaction:E cell  = E cathode  - E anode In this case, the MnO/Mn half-reaction is the cathode, and the Fe/Fe half-reaction is the anode.E cell  =  +1.51 V  -  +0.77 V E cell  = 0.74 VSo, the standard electrode potential for the given redox reaction in acidic medium is 0.74 V.