Question

What is the equilibrium constant k at 25 °C for an electrochemical cell when E° = 0.0165 V and n = 2? (F = 96,500 J/(V･mol), R = 8.314 J/(mol･K))

a) K = e⁰.⁰¹⁶⁵/⁰.⁰²⁵⁹
b) K = e⁰.⁰²⁵⁹/⁰.⁰¹⁶⁵
c) K = e⁰.⁰¹⁶⁵/⁰.⁰¹²⁹⁵
d) K = e⁰.⁰¹²⁹⁵/⁰.⁰¹⁶⁵

Answer 1

The equilibrium constant, K, can be calculated using the Nernst equation. Substituting the given values into the equation, we find that K is approximately equal to e^0.0259.

Step-by-step explanation:

The equilibrium constant, K, can be calculated using the Nernst equation. The equation is given by: K = e^((nE°)/(RT)), where n is the number of moles of electrons transferred, E° is the standard electrode potential, R is the gas constant, and T is the temperature in Kelvin.

Substituting the given values into the equation, we have: K = e^((2*0.0165)/(8.314*298))

Simplifying the expression, we find that the equilibrium constant K is approximately equal to e^0.0259.