Nernst's equation is given by
Ecell = E°cell - (RT/nF) * ln(Q)
Where:
Ecell = cell potential
E°cell = standard cell potential
R = gas constant
T = temperature in Kelvin
n = number of electrons transferred in the balanced redox reaction
F = Faraday constant
Q = reaction quotient
The equation can be derived from the Gibbs free energy equation:
ΔG = ΔG° + RT ln(Q)
Where:
ΔG = change in Gibbs free energy
ΔG° = standard Gibbs free energy change
R = gas constant
T = temperature in Kelvin
Using the equation ΔG = -nFEcell (where Ecell is the cell potential), we can substitute this into the equation above to get:
-nFEcell = -nFE°cell + RT ln(Q)
Dividing by -nF, we get:
Ecell = E°cell - (RT/nF) ln(Q)
This is Nernst's equation for calculating the cell potential of a cell under non-standard conditions.
Derive Nernst's equation for emf of a cell.
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