Nernst equation
Nernst Equation is a scientific equation used to find the reduction potential or voltage of an electrochemical cell. It is widely used in cell physiology and neurobiology. It is named after Walther Nernst. He was a German chemist who created this equation.
This equation can be used to check which combination of chemicals will be suitable to construct a powerful electric cell.
Expression
Nernst Equation:
[math]\displaystyle{ E_{cell}={E^o}- \frac{RT}{zF}\ln{Q} }[/math]
where
Ecell = Reduction potential or voltage of the electrochemical cell. In SI units, the voltage counts the one kilogram blocks you have to push one meter for each 6.2x1018 electrons you move across the cell. In a perfect world, every time a 9 volt battery moves 6.2x1018 electrons, we could harness the slow-moving electrons to move 9 blocks one meter.
E = Standard potential of the cell. It is the reduction potential of the cell or voltage under standard conditions (Temperature = 298 Kelvin, Pressure = 1 bar).
R = Gas constant. It is an important constant used in thermodynamics. Its value is 8.314 J.K-1.mol-1.
T = Temperature of the electrochemical cell in Kelvin.
z = Number of moles of electrons that got transferred when reduction took place.
F = Faraday constant. It is equal to the charge carried by 1 mole of electrons. Faraday constant = 96,485.3329 s Ampere/mole.
Q = Reaction quotient of the chemical reaction that is driving the cell.
Equilibrium
When the reduction potential of a cell = 0 V, it is in equilibrium. At equilibrium, the reaction quotient Q = Keq (equilibrium constant).