Consider the following unbalanced redox reaction: MnO4- + S2O32- → Mn2+ + SO42- What is the reduction half-reaction? MnO4- → SO42- MnO4- → Mn2+ S2O32- → SO42- S2O32- → Mn2+

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Consider the following unbalanced redox reaction: MnO4- + S2O32- → Mn2+ + SO42- What is the reduction half-reaction? MnO4- → SO42- MnO4- → Mn2+ S2O32- → SO42- S2O32- → Mn2+

Chemistry
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Which one do you think it is?
We know that it is not A or D a half reaction shows the reaction for one element so it wouldn't chand it either needs to be Mn or S only it can't be Mn and S
We are looking for the reduction portion so reduction gains electrons, oxidation loses electrons

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MnO4- In order to get the -1 charge Mn has a charge of +7 and on the other side of the reaction Mn has a charge of +2 it is gaining electrons since it's getting closer to being negative so it is being reduced
Do you understand @ajeecutie ?
yep

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