The electrode potential of the following half cell at 298 K X X 2 + 0 . 001 M ‖ Y 2 + 0 . 01 M Y is _____ × 10 - 2 V (Nearest integer) Given : E X 2 + ∣ X 0 = - 2 . 36 V E Y 2 + Y 0 = + 0 . 36 V 2 . 303 RT F = 0 . 06 V

Step-by-step solution

The net cell reaction can be written as follows, X + Y 2 + → Y + X 2 + E cell 0 = E cathode 0 - E anode 0 (Both are SRP values) E Cell 0 = 0 . 36 - - 2 . 36 = 2 . 72   V Now, the Nernst equation is, E cell = E cell 0 - 0 . 06 n log X 2 + Y 2 + n = The number of electrons involved in the net reaction. E Cell = 2 . 72 - 0 . 06 2 log 0 . 001 0 . 01 = 2 . 72 + 0 . 03 = 2 . 75   V = 275 × 10 - 2   V