Question

In the redox reaction: Cr2O72- + Fe2+ --> Cr3+ + Fe3+. What would the balanced reaction look like, and would CrO72- be the Reducing Agent, and Fe2+ be the Oxidizing Agent?

Answer 1

Dichromate is the oxidizing agent....

Explanation:

And ferrous ion is the species that is oxidized....

And we use the method of half-equations..

`"Reduction half equation:"`

`underbrace(Cr_2O_7^(2-))_"red-orange" + 14H^+ + 6e^(-) rarr 2Cr^(3+) + 7H_2O(l)`

`"Oxidation half equation:"`

`Fe^(2+) rarr Fe^(3+) +e^(-)`

And we add the equations together in such a way that the electrons are eliminated...

`6Fe^(2+) +Cr_2O_7^(2-) + 14H^+rarr 6Fe^(3+) +2underbrace(Cr^(3+))_"green" + 7H_2O(l)`

Is this balanced with respect to mass and charge?