L13 Equilibrium electrochemistry - The Nernst equation

Why is this model simplistic

It doesn’t take into account he different charges on the reduced/oxidised species

Changing the point of equilibrium by varying electric potential

Combining half-equations to form a chemical equation

Half cell potentials and the standard hydrogen electrode

Measuring half cell potentials and writing equations and descriptions of the cell

Highest potential goes on RHS

Other reference electrodes

Effect of pH on potential

Using protons in the equation means that pH is going to be involved in some way

Thermodynamics of half-cell reactions

In this case the entropy change involving the copper is much larger as we are producing a solid.

Electrochemical cells

Combining half cells to make full cells

Splitting the full cell reaction into half reactions

how do you reverse the direction of a reaction using electrochemistry

Adding a power supply allows reversal of the current compared to the direction it would go with a simple resistor

Nernst equation for a cell at standard conditions

Nernst equation for a full cell at non-standard conditions

Nernst equation for a half cell reaction

Nernst equation combining 2 half cells example

Concentration cells

Same reactants, different concentrations