Help with writing half reactions for the following

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To write the half-reactions for the redox process involving Fe2+ and MnO4- in acidic solution, identify the oxidation and reduction components. Fe2+ is oxidized to Fe3+, while MnO4- is reduced to Mn2+. The half-reaction for oxidation is Fe2+ → Fe3+ + e-, and for reduction, it is MnO4- + 8H+ + 5e- → Mn2+ + 4H2O. Balancing the overall reaction requires multiplying the half-reactions to ensure equal electron transfer. This classic redox titration is commonly found in educational resources.
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1. Fe2+ + MnO4- -> Fe3+ + Mn2+ (acidic solution)


2. I need to write a half reaction for the oxidation and reduction process and I am totally lost. If I could have help on this one, maybe I will understand how to complete the balance of my work.
 
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mkrupich said:
1. Fe2+ + MnO4- -> Fe3+ + Mn2+ (acidic solution)


2. I need to write a half reaction for the oxidation and reduction process and I am totally lost. If I could have help on this one, maybe I will understand how to complete the balance of my work.


Remember, lose electrons oxidized, gain electrons reduced. What indicates the electron movement for any reaction? After you figure that out, break the reaction into half-reactions.
 
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Break the answer down:

What is being reduced?
What is being oxidised?
Write the half equation for the reduction
Write the half equation for the oxidation
Multiply up the 2 half equations so they balance

This is such a classic redox titration that you will find it in any school textbook
 
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