## Bronsted Neutralization Reaction

chloewinnett1L
Posts: 55
Joined: Fri Sep 28, 2018 12:20 am

### Bronsted Neutralization Reaction

The solutions manual says that the proper redox reaction for the formation of water from hydronium and hydroxide ions involves the two following reactions:
$O_{2}(g)+4H^{+}(aq)+4e\rightarrow 2H_{2}O(l)$ (cathode) and $O_{2}(g)+2H_{2}O(l)+4e\rightarrow 4OH^{-}$ (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:
$2H^{+}(aq)+2e\rightarrow H_{2}$ (cathode) and $2H_{2}O(l)+2e\rightarrow H_{2}(g)+2OH^{-}(aq)$ (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.

Tiffany_Cacy_3D
Posts: 70
Joined: Fri Sep 28, 2018 12:24 am

### Re: Bronsted Neutralization Reaction

I did the same exact thing and got the same answer. I think as long as everything cancels out correctly it should be the same. On the test there will only be a certain number of reactions to choose from as well so I think it will be more clear which reactions we are supposed to use.