Question: Given: Ferrous ion ( Fe 2+ ) is converted into ferric hydroxide solid, Fe(OH) 3(s) , and dichromate ion (Cr 2 O 7 2- )
Given: Ferrous ion ( Fe2+ ) is converted into ferric hydroxide solid, Fe(OH)3(s), and dichromate ion (Cr2O72-) is converted into chromium dihydroxo complex, Cr(OH)2+.
_Fe2+ + _Cr2O72- => _Fe(OH)3(s) + _Cr(OH)2+ (unbalanced)
Required:
a) Balance this redox reaction. Required: .
1) Show calc.s for determining oxid. state of all species that undergo a change in oxid. state.
2) Indicate total number of e-s stripped from each atom of reductant, and the total number accepted by each atom of the oxidizing agent.
3) show how many moles of oxidant are needed to balance e-s removed vs gained.
4) Remember to balance the other atoms and the charge. Assume that the reaction takes place under acidic conditions.
b) Which element is the oxidizing agent (oxidant)? Reducing Agent (reductant)?
c) Which element is being oxidizing? Reduced?
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