23.5 predictions from electrode potentials

how to use standard electrode potentials to make predictions about feasibility

a reaction should take place between an oxidising agent and a reducing agent, provided that the oxidising agent has a more positive standard electrode potential value that the redox system of the reducing agent

which way are half cells written in the table

reduction is always the forwards reaction

how to gain the oxidation overall equation from two half equations

reversing the equilibrium then forming the equation

limits of making predictions using standard electrode potential values

some reactions may have a large activation energy

the concentration may not be exactly 1mol/dom³

other conditions may not be standard

what happens if the concentration of Zn2+ is greater than 1mol/dm³

the equilibrium will shift to the right, removing electrons from the system making the electron potential less negative