Consider the following oxidation-reduction reaction: I(aq)+Cu+(aq)IO3(aq)+Cu(s)

Question

Consider the following oxidation-reduction reaction:

I(aq)+Cu+(aq)IO3(aq)+Cu(s)

A) What are the initial and final oxidation states of iodine? B) What are the initial and final oxidation states of copper? C) What element is oxidized? D) What is the reducing agent? E) What element is reduced? F) What is the oxidizing agent? G) Give the atom- and electron-balanced oxidation half-reaction occurring in acidic solution. H) Give the atom- and electron-balanced reduction half-reaction occurring in acidic solution.

Explanation / Answer

a) initial oxidation state of iodine is -1

final oxidation stae of iodine is +5

b)initial oxidation state of copper is +1

final oxidation stae of copper is 0

c) Iodine is oxidised (increase in oxidation number)

d) the reducing agent is I- (aq) as it reduced Cu+1 to Cu(o)

e) The element reduced is copper

f) the oxidising agent is Cu+ as it oxidised I- to IO3-

g) oxidation half reaction

I- (aq) + 3H2O(l) ----------> IO3-(aq) + 6H+(aq) + 6e-

h) reduction half reaction

Cu+ (aq) --------> Cu(s) + e-

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