Hg + 2Cr3+Hg2+ + 2Cr2+ In the above reaction, the oxidation state of chromium changes from to . How many electrons are transferred in the reaction?

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3Fe(s) + Cr₂O₇^2-(aq)+14H⁺(aq) ?3Fe²⁺(aq) + 2Cr³⁺(aq) +7H₂O(l) ?^o=1.77V

True or False? and why?!

The oxidation state of chromium in dichromate is +3.
The oxidizing agent is Cr³⁺ (aq)
The oxidation state of oxygen changes from 0 to -2.
The reducing agent is Cr³⁺ (aq)
The chromium half-reaction takes place in an acidic solution.
The highest oxidation state for chromium in this reaction is +6

For the reaction, shown below, determine which statements are True and which are False and explain.
3Fe(s) + Cr2O72-(aq) +14H+(aq) â 3Fe2+(aq) + 2Cr3+(aq) + 7H2O(l) Î¾o=1.77V

1) The iron half-reaction takes place in an acidic solution.
2)The oxidation state of chromium in dichromate is +3.
3)The highest oxidation state for chromium in this reaction is +7
4)The oxidizing agent is dichromate (Cr2O72-).
5)The reducing agent is dichromate (Cr2O72-).
6)The oxidation state of oxygen changes from 0 to -2.

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Hg + 2Cr3+Hg2+ + 2Cr2+ In the above reaction, the oxidation state of chromium changes from to . How many electrons are transferred in the reaction?

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