November 01, 2024, 04:16:36 AM
Forum Rules: Read This Before Posting


Topic: How do you find the products of a redox equation?  (Read 1835 times)

0 Members and 1 Guest are viewing this topic.

Offline yeiure

  • Very New Member
  • *
  • Posts: 2
  • Mole Snacks: +0/-0
How do you find the products of a redox equation?
« 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!  :)
               

Offline AWK

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 7978
  • Mole Snacks: +555/-93
  • Gender: Male
Re: How do you find the products of a redox equation?
« Reply #1 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.
AWK

Offline yeiure

  • Very New Member
  • *
  • Posts: 2
  • Mole Snacks: +0/-0
Re: How do you find the products of a redox equation?
« Reply #2 on: February 21, 2016, 12:09:30 AM »

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

Sponsored Links