Consider the following unbalanced redox reaction: Bi_2O_4(aq) + I^-(aq) rightarr

Question

Consider the following unbalanced redox reaction: Bi_2O_4(aq) + I^-(aq) rightarrow BiO^+(aq) + IO_3^_(aq) (a) Balance the corresponding half reactions in acidic conditions using the lowest possible whole number coefficients. (Enter coefficients for one and zero. Blanks will be marked incorrect.) Bi_2O4(aq) + H_2O(l) + OH^-(aq) + H^+(aq) + e^- rightarrow BiO^+(aq) + H_2O(l) + OH^-(aq) + H^+(aq) + e^- I^-(aq) + H_2O(l) + OH^-(aq) + H^+(aq) + e^- rightarrow IO_3^-(aq) + H_2O(l) + OH^-(aq) + H^+(aq) + e^- (b) Using the results from part (a), balance the full reaction in acidic conditions with the lowest possible whole number coefficients. (Enter coefficients for one and zero. Blanks will be marked incorrect.) Bi_2O_4(aq) + I^-(aq) + H_2O(l) + OH^-(aq) + H^+(aq) rightarrow BiO^+(aq) + IO_3^-(aq) + H_2O(l) + OH^-(aq) + H^+(aq)

Explanation / Answer

a) reduction half reaction is

Bi2O4(aq) + 4H+(aq) + 2e- --------------> 2 BIO+(aq) + 2 H2O (l)

oxidation half reaction is

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

b) The full balanced equation is obtained by multiplying the Reduction hhalf reaction with 3 and adding the oxidation half reaction.

Full equation is

3 Bi2O4(aq) + 6H+(aq) + I- (aq) -----------> 6BiO+(aq) + 3H2O (l) + IO3- (aq)

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