Bronsted Neutralization Reaction
Posted: Thu Mar 14, 2019 9:41 pm
The solutions manual says that the proper redox reaction for the formation of water from hydronium and hydroxide ions involves the two following reactions:
(cathode) and
(anode).
Using these two reactions gives you an overall standard cell potential of +0.83V.
However, I used the following two reactions to obtain water:
(cathode) and
(anode)
and ended up with the exact same standard cell potential, +0.83V.
My question is, are both of these routes valid? As far as I can tell, the only difference between the two is that the first path uses oxygen gas as an intermediate and the second path uses hydrogen gas as an intermediate.
Using these two reactions gives you an overall standard cell potential of +0.83V.
However, I used the following two reactions to obtain water:
and ended up with the exact same standard cell potential, +0.83V.
My question is, are both of these routes valid? As far as I can tell, the only difference between the two is that the first path uses oxygen gas as an intermediate and the second path uses hydrogen gas as an intermediate.