Calculate the standard cell potential (E∘) for the reaction X (s) + Y + (aq) →X + (aq) + Y (s) if K = 5.59*10-3.

E° = - 0.133 V

Explanation:

In the reaction:

X (s) + Y⁺ (aq) → X⁺ (aq) + Y (s)

1 electron is transferred from X to Y

Now, using Nernst equation:

E° = RT / nF ln K

Where R is gas constant (8.314 J/molK), T is absolute temperature (Usually 298.15K), n are transferred electrons (1, for the reaction), F is faraday constant (96485C/mol) and K is equilibrium constant (5.59x10⁻³)

Replacing:

E° = 8.314 J/molK*298.15K / 96485C/mol*1 ln 5.59x10⁻³

E° = - 0.133 V