- #1
Big-Daddy
- 343
- 1
The partial pressures of O2 and H2 in the atmosphere above water are typically very low indeed, so why is it we don't see the equilibria 2 H2O = O2 (g) + 4H+ + 4e- and 2 H+ + 2e- = H2 (g) occurring whenever we have a beaker of water (if this was observed then the H+ concentration would be changing even in pure water)? Since K=1 for the 2 H+ + 2e- = H2 (g) and the partial pressure of H2 in air is incredibly small, shouldn't this reaction be moving forward?
And what about the redox reactions water can undergo involving hydroxide ions rather than protons? Don't these equilibria exist too? (e.g. 4H2O + 4e- = 2 H2 (g) + 4 OH-)
And what about the redox reactions water can undergo involving hydroxide ions rather than protons? Don't these equilibria exist too? (e.g. 4H2O + 4e- = 2 H2 (g) + 4 OH-)
Last edited: