20. Electrochemistry

Calculate the equilibrium constant for the following reaction at 25ºC. 

Fe (s) + I₂ (s)  →  Fe²⁺ (aq) + 2 I ^– (aq)

Given the following reduction potentials: 

Fe²⁺(aq) + 2 e^–  →. Fe (s)                          E°_red = – 0.45 V

I₂ (s) + 2 e^–  →. 2 I ^– (aq)                           E°_red = + 0.54 V

A cell has a standard cell potential of +0.177 V at 298 K. What is the value of the equilibrium constant for the reaction

(a) if n = 1?

At 298 K a cell reaction has a standard cell potential of +0.17 V. The equilibrium constant for the reaction is 5.5 × 10⁵. What is the value of n for the reaction?