If standard reduction potential of Zn, Ni and Fe are -0.76 , V , -0.23 , V and -0.44 , V respectively. For the reaction (Stated below) to be spontaneous find out electrodes X and Y considering above electrode potentials X _ (s) + Y ⁺²_ (aq) X ⁺²_ (aq) + Y _ (s)

Step-by-step solution

For the given reaction X _ (s) + Y ⁺²_ (aq) X ⁺²_ (aq) + Y _ (s) , X undergoes oxidation and acts as the anode, while Y undergoes reduction and acts as the cathode. For the reaction to be spontaneous, the standard cell potential E^ _ cell must be positive. E^ _ cell = E^ _ cathode - E^ _ anode = E^ _ Y - E^ _ X > 0 This implies E^ _ Y > E^ _ X . Given standard reduction potentials: E^ _ Zn = -0.76 , V E^ _ Ni = -0.23 , V E^ _ Fe = -0.44 , V Checking the given options: If X = Ni, Y = Fe: E^ _ cell = -0.44 - (-0.23)