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<a https://www.thestudentroom.co.uk/showthread.php?t=7467335'> Year 12s: what will be the first way you research your future options? >>
<a https://www.thestudentroom.co.uk/showthread.php?t=7467335'> Year 12s: what will be the first way you research your future options? >>
<a https://www.thestudentroom.co.uk/showthread.php?t=7467335'> Year 12s: what will be the first way you research your future options? >>

Redox Walk Through Please :)

Please help me solve this step by step -
Half Reactions -
NO3-+ 4H+ + 3e- ----> NO + 2H2O
Fe2+ + 2e- ------> Fe

The equation is
NO3-+ 4H+ + Fe -----> NO + H2O + Fe2+

I understand some things, but not knowing if I can add H+, should I add the electrons from the half reactions in from the start or leave until the end? As if we include from the start it unbalances the overall charge.
Also in this both the NO and Fe are being oxidised right?
Original post by benzenee
Please help me solve this step by step -
Half Reactions -
NO3-+ 4H+ + 3e- ----> NO + 2H2O
Fe2+ + 2e- ------> Fe

The equation is
NO3-+ 4H+ + Fe -----> NO + H2O + Fe2+

I understand some things, but not knowing if I can add H+, should I add the electrons from the half reactions in from the start or leave until the end? As if we include from the start it unbalances the overall charge.
Also in this both the NO and Fe are being oxidised right?


The procedure is to multiply both of the half equations by suitable factors to make the electrons equal BEFORE you add them together.

The equation you have written is neither correct for atoms nor charges...
Reply 2
Avatar for Big-Daddy
Big-Daddy
13
Read "redox equations" on ChemGuide.
Reply 3
Avatar for saurabhrai
saurabhrai
You have to follow these two criteria first:

1. For a Redox reaction charge on both side should be balanced.

2. And like a normal chemical equation balancing atoms should also be balanced.
(edited 10 years ago)

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