Question 1

What is the Nernst equation?

Accepted Answer

The Nernst equation relates the cell potential to the standard cell potential and the reaction quotient: E = E° - (RT/nF)ln(Q). At 25°C, this simplifies to E = E° - (0.0592/n)log(Q) using log base 10.

Question 2

What are R and F in the equation?

Accepted Answer

R is the universal gas constant (8.314 J/(mol·K)) and F is Faraday's constant (96,485 C/mol), which represents the charge of one mole of electrons.

Question 3

What happens when Q = 1?

Accepted Answer

When Q = 1, ln(Q) = 0, so E = E°. This means the cell potential equals the standard potential when all species are at standard conditions (1 M, 1 atm).

Question 4

How is the Nernst equation related to equilibrium?

Accepted Answer

At equilibrium, E = 0 and Q = K (equilibrium constant). This gives: E° = (RT/nF)ln(K), allowing you to calculate K from E° or vice versa.

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