In Class Example
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In Class Example
Can anyone explain the end result for the reaction Dr. Lavelle did in class with permanganate and iron?
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Re: In Class Example
The reaction of the permanganate ion with Fe2+ in water is written as:
8H+ + MnO4- + 5Fe2+ --> Mn2+ + 5Fe3+ + 4H2O
This reaction can show that MnO4- is the oxidizing agent because it is reduced to Mn2+ and Fe2+ is the oxidizing agent because it is oxidized to Fe3+. This can be seen in the half-reactions:
oxidation: 5Fe2+ --> 5Fe3+ + 5e-
reduction: 8H+ + MnO4- + 5e- --> Mn2+ + 4H2O
Here Mn is reduced from +7 charge to +2 charge.
8H+ + MnO4- + 5Fe2+ --> Mn2+ + 5Fe3+ + 4H2O
This reaction can show that MnO4- is the oxidizing agent because it is reduced to Mn2+ and Fe2+ is the oxidizing agent because it is oxidized to Fe3+. This can be seen in the half-reactions:
oxidation: 5Fe2+ --> 5Fe3+ + 5e-
reduction: 8H+ + MnO4- + 5e- --> Mn2+ + 4H2O
Here Mn is reduced from +7 charge to +2 charge.
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Re: In Class Example
He just broke the reaction up into two half reactions; it is not necessarily an end result, but a breakdown of what is going on in one redox reaction.
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Re: In Class Example
I don't think you have to do it this way, but it makes things a lot easier to see and understand.
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