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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: yeiure on February 20, 2016, 07:45:03 PM

Title: How do you find the products of a redox equation?
Post by: yeiure on February 20, 2016, 07:45:03 PM
I can balance redox equations fairly easily, but I just can't seem to finish the equation... :-[
For example, MnO4- + H2O2  :rarrow: Mn2+ +  ??
I know the full equation, but I don't know what steps to take to get there
Any help would be very appreciated!  :)
               
Title: Re: How do you find the products of a redox equation?
Post by: AWK on February 20, 2016, 08:35:36 PM
MnO4-  :rarrow:  Mn2+
this half reaction needs [H+] or [H3O+] on the left side
H2O2 is oxidized  :rarrow: then forms water H2O and oxygen O2
That's all.
But this reaction has hidden agenda. Mn2+ catalytically decomposes H2O2. This means you can add hydrogen peroxide on the left side obtaining additional water and oxygen on the right side. In this manner you can form infinity numbers of balanced reactions.
Title: Re: How do you find the products of a redox equation?
Post by: yeiure on February 21, 2016, 12:09:30 AM

Quote from: AWK on February 20, 2016, 08:35:36 PM
MnO4-  :rarrow:  Mn2+
this half reaction needs [H+] or [H3O+] on the left side
H2O2 is oxidized  :rarrow: then forms water H2O and oxygen O2
That's all.
But this reaction has hidden agenda. Mn2+ catalytically decomposes H2O2. This means you can add hydrogen peroxide on the left side obtaining additional water and oxygen on the right side. In this manner you can form infinity numbers of balanced reactions.

Thank you so much for your *delete me*! I understand it now :D