Now I'm confused... couldn't all of them because reversing the sign of each reducing agent in the list and adding it to +1.82 gives a positive Ecell value?
For question 2: change in temp, pressure or concentration. In each case the equilibrium position could move and this will affect the electrode potential.
<--> is my beautiful representation of a reversible reaction
2. Suggest two factors that might prevent a reducing agent from being as effective as the electrode potentials might seem to suggest.
This is from the January 2003 paper - If anyone knows where an online mark scheme is, can they let me know.. cheers
answer 1..zinc metal. it will reduce the Co3+ to Co2+ because when its half equaction is reversed and added to Co3+ + e-= Co 2+, the Ecell= +0.76+ 1.82v, which is positive , so the reaction will take place. and it will reduce Co 2+ to Co, as Ecell = +0.76 + (-0.28) = +0.48 v is also positive..
answer 2.. non standard condition and higher activation energy