Standard electrode potentials

E°cell value from strongest to weakest oxidising agents of K, Cl2, Al and I2

strongest = most easily reduced i.e gains electrons

Cl2(+1.68V), I2(+0.54V), Al, K

strongest to weakest: Ba(-2.94V), Ni(-1.68V), Ag, F2

How to calculate E°cell:

E°cell = E°red - E°ox

if positive = reaction is spontaneous

if negative = reaction is not spontaneous

*A voltage greater than the E°cell would need to be applied to get the reaction to occur

calculate E°cell of Zn and I2:

Describe the purpose of the standard electrode potential table.

The table provides a comparison of the ease for reduction to occur by giving half-cell potentials and allows us to work out which species is reduced and which is oxidised for a spontaneous reaction to occur.

Annotate the table below with key features: