4 posts • Page 1 of 1
In the solution manual, it says to choose the reduction reaction with most positive standard reduction potential for the cathode and choose reduction reaction with most negative standard reduction potential for the anode. But they choose Ni2+ reaction for cathode which has E=-0.23V and choose H2O reaction for anode which has E=+1.23V. Using their reasoning described, shouldn't the cathode reaction be the H2O reaction since it is the most positive standard reduction?
Chem_Mod wrote:The reduction half reaction you should be considering for water is 2H2O + 2e —> H2 + 2OH- with Ecell= -0.83 V
The half reaction you are thinking of is for the reduction of O2 into water
I am also a bit confused on this question because the book chooses the cathode as Ni2+(aq) +2e- ->Ni(s) instead of the reduction half reaction for water with Ecell = -0.83V, and the anode as the oxidation of water 2H2P(l)-> O2(g) = 4H+ (aq) +4e- with Ecell= +1.23V. Why is that?
Who is online
Users browsing this forum: No registered users and 4 guests