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OpenStudy (anonymous):
Identify the oxidizing agent and the reducing agent for 4Li(s) + O_2 (g) to 2Li_2O(s).
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OpenStudy (anonymous):
\[4Li _{(s)}+O _{2}(g) \rightarrow 2Li _{2}O _{(s)}\]
OpenStudy (anonymous):
Really need help trying to understand redox reactions.
OpenStudy (anonymous):
http://answers.yahoo.com/question/index?qid=20100215222246AA9pFud this misht help you :)
OpenStudy (anonymous):
thanks didn't try yahoo yet
OpenStudy (anonymous):
no problem
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OpenStudy (aaronq):
Li is being oxidized and thus is the reducing agent i know this because oxygen always has a -2 oxidation state and since it's oxidation state in diatomic oxygen is zero, it was reduced, and so oxygen is the oxidizing agent
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