Chemistry Forum

Develop halfreactions MnO4 - to MnO2 MnO4 - + 2 H2O => MnO2 + 4 OH- Balance chargse MnO4 - + 2 H2O + 3 e- => MnO2 + 4 OH- Reduction SO3 2- to SO4 2- SO3 2- + 2 OH- => SO4 2- + H2O Balance of charge SO3 2- + 2OH - => SO4 2- + H2O + 2e- Oxidation Make electrons equal 2 MnO4 - + 2 H2O => + 6 e- =>2 MnO...

An example for redox reaction is as follows: 2 Al +3 Br2 -> Al2Br6 In this reaction Bromine is been oxidized and Aluminum is being reduced Its opposit Aluminium is oxidized and Bromine reduced. Al = Al 3+ 3 e- as you mentioned loosing electrons. Br2 + 2 e- ´2 Br- Bromine gain electrons.

wrong potential choosen

You choose Fe2+ to Fe3+ with 0,77 V

but you have Fe and Fe3+ in your cell it has -0,036 V

between there is also Fe and Fe 2+ with -0.402 V

Why not post your question here, more help can be received.

using = and >

gives =>

like A + B => C+ D

bejoy wrote:
An example for redox reaction is as follows:

2 Al +3 Br2 -> Al2Br6

In this reaction Bromine is been oxidized and Aluminum is being reduced

I would think about it, its the opposit Aluminium gets oxidiesd

Al => Al3+ + 3 e-

Bromine gets reduced