Question

Which from following equations is correct for relation between standard cell potential and equilibrium constant?

• A. Ecell =$\frac {0.0592}{n}$ log10 K
• B. Ecell = log10 K$\frac {n}{(0.0592)}$
• C. E0cell = $\frac {0.0592}{n}$ log10 K
• D. Ecell = log10 K$\frac {n}{0.0592}$

Answer 1

Answer: (C)

E0cell = $\frac {0.0592}{n}$ log10 K

Answer 2

The correct equation for the relation between standard cell potential (E°cell) and equilibrium constant (K) is:
E0cell = $\frac {0.0592}{n}$ log10 K
This equation is known as the Nernst equation and is used to calculate the cell potential of an electrochemical cell under non-standard conditions. In the equation, "n" represents the number of moles of electrons transferred in the balanced redox reaction. Therefore, the correct answer is (C) E0cell = $\frac {0.0592}{n}$ log10 K.