Sb2O5 + 4Fe2++ 6H+4Fe3+ + 2SbO++ 3H2O name of the element oxidized: name of the element reduced: formula of the oxidizing agent: formula of the reducing agent?

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Answer 1 · 2018-05-17T06:15:13

You got #Sb(+V)# reduced to #Sb(+III)#...

#Sb_2O_5 + 6H^+ +4e^(-) rarr 2SbO^(+) + 3H_2O(l)# #(i)#

Charge and mass are balanced so this is kosher...and there is a corresponding oxidation reaction....

#Fe^(2+) rarr Fe^(3+) + e^(-)# #(ii)#

And we add the equations together in such a way that the electrons, virtual particles of convenience, are eliminated......#(i)+4xx(ii)# gives....

#4Fe^(2+)+Sb_2O_5 + 6H^+ +4e^(-) rarr 4Fe^(3+) + 2SbO^(+) + 3H_2O(l)+4e^(-)#

... gives finally....

#4Fe^(2+)+Sb_2O_5 + 6H^+ rarr 4Fe^(3+) + 2SbO^(+) + 3H_2O(l)#

Are charge and mass balanced? If the answer is NO, then we cannot accept the reaction as a model of reality.