Predictions from electrode potentials

If a redox system had a more positive E^o value what does this mean?

the oxidising agent on the left will react with the reducing agents on the right of the other redox systems

How do you write overall equations?

combing the half equations:

redox system with more positive E^o value will react from left to right

redox system with less positive E^o value will react from right to let

What are the limitations of predicting using E^o values?

give no indication of the rate of the reaction - may have large activation energy

actual conditions may be different from the standard conditions

standard elctrode potentials apply to aqueous equilbiria

Why is concentration a limitation of predicting using E^o values?

standard electrode potentials are measured using 1mol dm-3

changing concentrations will cause equilibrium to shift and make electrode potentials more or less negative

When is a reaction feasible?

the standard cell potential, E^ocell, is positive