IO3-(aq) + Fe2+(aq) ⇌ Fe3+(aq) + I2(aq)
▪ Anode → oxidation
▪ oxidation half-reaction happens in the anode solution
▪ losing electrons → becoming more positive
Anode: Fe2+(aq) ⇌ Fe3+(aq)
▪ Cathode → reduction
▪ reduction half-reaction happens in the anode solution
▪ gaining electrons → becoming more negative
IO3‒(aq) ⇌ I2(aq)
▪ Balance I:
2 IO3‒(aq) ⇌ I2(aq)
▪ Add 1 H2O: 1 O
2 IO3‒(aq) ⇌ I2(aq) + 6 H2O(l)
▪ Add 1 H+: 1 H
2 IO3‒(aq) + 12 H+(aq) ⇌ I2(aq) + 6 H2O(l)
O.S. of I in IO3‒ = +5
O.S. of I in I2 = 0 (standard state)
Cathode: 2 IO3‒(aq) + 12 H+(aq) ⇌ I2(aq) + 6 H2O(l)
Sketch the galvanic cells based on the following overall reactions. Show the direction of electron flow, the direction of ion migration through the salt bridge, and identify the cathode and anode. Give the overall balanced equation. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm.
a. IO3- (aq) + Fe2+ (aq) ⇌ Fe3+ (aq) + I 2 (aq)
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.