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In a cell, the following reactions take place Fe 2 + → Fe 3 + + e -    E o Fe 3 + / Fe 2 + = 0 . 77   V 2 I - → I 2 + 2 e -    E I 2 / I - 0 = 0 . 54   V The standard electrode potential for the spontaneous reaction in the cell is x × 10 - 2   V   at   298   K . The value of x is - (Nearest Integer)

Correct answer

0

Step-by-step solution

The electrode which has more reduction potential will get reduced in spontaneous reaction in the cell. So, spontaneous reaction will be 2 Fe 3 + aq + 2 I - aq → 2 Fe 2 + aq + I 2 Iron will act as cathode and Iodine will act as anode. E 0 cell = E 0 RP C - E 0 RP A = 0 . 77 - 0 . 54 = 0 . 23   V = 23 × 10 - 2   V

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