Asked by Parker
I need to calculate the redox potential for the following:
1/2 O2 + 2H+ + 2e- <-> H2O
I'm using the formula
E = E'_0 + RT\nF ln ([electron acceptor]/[electron donor])
The electron acceptor is H+, so I can use the concentration of that which is indicated by the pH.
However, the electron donor seems to be H2O. The molarity of pure water is 55.346 M. Am I really supposed to use that? I have a suspicion that I'm not supposed to do that.
1/2 O2 + 2H+ + 2e- <-> H2O
I'm using the formula
E = E'_0 + RT\nF ln ([electron acceptor]/[electron donor])
The electron acceptor is H+, so I can use the concentration of that which is indicated by the pH.
However, the electron donor seems to be H2O. The molarity of pure water is 55.346 M. Am I really supposed to use that? I have a suspicion that I'm not supposed to do that.
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