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frozonecom
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Homework Statement
[tex]H_{2} + O_{2} \rightarrow H_{2}O[/tex]
Homework Equations
The Attempt at a Solution
Well, my classmates insist that H= +1 and O= -2 (in the products side)
so, my Hydrogen will be my Reducing agent because it underwent Oxidation and my Oxygen will be my Oxidizing agent because it underwent Reduction
Reduction: [tex]O_{2} \rightarrow H_{2}O[/tex]
Oxidation: [tex]H_{2} \rightarrow H_{2}O[/tex]
From here on, I can't understand anything.
Well, I need to know what to do here. I was told by this video:
https://www.youtube.com/watch?v=AyKiYz-YpSw
Particularly in 4:09, in that problem, she said that [tex]H_{2}O[/tex] has a charge of 0. I know that Hydrogen and Oxygen in the reactants side has 0 charge / oxidation number too because it is in its "pure" form. So, is this equation "BALANCE-able" ??
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