The equation relating the standard cell potential of a voltaic cell to the stand

Question

The equation relating the standard cell potential of a voltaic cell to the standard reduction potential of the cathode and anode reactions is the following. E_cell^0 - E_cathode^0 - E_anode^0 In this equation E_cell^0 is the standard cell potential, E_cathode^0 is the standard reduction potential of the cathode reaction, and E_anode^0 is the standard reduction potential of the reverse of the anode reaction (the reduction corresponding to the reverse of the oxidation reaction). Use this relationship to solve the problem below. The standard reduction potential for Ni^2+ (aq) is -0.26 V. The half-reaction for the reduction of Ni^2+ (aq) is the following. Ni^2+ (aq) 2 e^- rightarrow Ni(s) The standard reduction potential for Cr^3+ (aq) is -0.74 V. The half-reaction for the reduction of cr^3+ (aq) is the following. Cr^3+ (aq) + 3e^- rightarrow Cr(s) Using this information, calculate E_cell^0 for the voltaic cell powered by the following spontaneous redox reaction. 3Ni^2+ (aq) + 2 Cr(s) rightarrow 2 Cr^3+ (aq) + 3 Ni(s) V

Explanation / Answer

E cell= E cathode–E anode

E cathode = -0.26V

E anode = -0.74V

therefore E cell= -0.26V -(-0.74V)

                        = + 0.48V

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