Write balanced half-reactions for the following redox reaction: Cr2O2-7(aq) 7H2O(l) 6Fe2 (aq) 2Cr3 (aq) 14OH-(aq) 6Fe3 (aq)

Explanation:

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In this case, according to the given information, it turns out possible for us to write out the balanced half reactions by considering that chromium is being reduced and iron oxidized from 6+ to 3+ and 2+ to 3+ respectively, in such a way, we have:

Now, we insert the appropriate amount of water molecules and the carried electrons in order to balance both oxygen and consequently hydrogen:

Which is further transformed to the equation given in the problem due to the electron balance.

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