|
spock
|
 |
« Reply #1 on: August 08, 2008, 06:59:54 AM » |
|
Not sure about common gases, but I do know that hydrogen peroxide (usually found in water solutions) can act as both an oxidizing and reducing agent.
The hydrogen peroxide can undergo oxidation (the loss of electrons) according to the following 1/2 reaction:
2 H2O2 --> H2O + O2 + 2 H+ + 2 e-
It can undergo reduction according to the following:
H2O2 + 2e- ---> 2 OH-
The two reactions occur simultaneously in solutions of H2O producing a net reaction of
2 H2O2 --> 2H2O + O2
This is why H2O2 solutions tend to go back over time.
The halogens likely undergo both oxidation and reduction. Cl2 is a common oxidizing agent (that is it undergoes reduction or the gain of electrons) forming Cl-. Since ions of Cl containing positive oxidation states exist (ClO3-, ClO2-, ClO-), there must be some circumstances where the Cl2 is reduced as well.
|
