Consider the following unbalanced redox reaction: Br (aq) + ClO 4 (aq) BrO (aq)

Question

Consider the following unbalanced redox reaction:

Br(aq) + ClO4(aq) BrO(aq) + ClO3(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.)

Half equations

(b) Using the results from part (a), balance the full reaction in acidic conditions with the lowest possible whole number coefficients.

(c) Using the results from part (b), balance the full reaction in basic conditions with the lowest possible whole number coefficients.
(Enter coefficients for one and zero. Blanks will be marked incorrect.)

Explanation / Answer

(a) Br- + ClO4- ---> BrO- + ClO3-

First half reaction

Br- ---> BrO-

balance O,

Br- + H2O --> BrO-

balance H,

Br- + H2O ---> BrO- + 2H+

add e-'s,

Br- + H2O ---> BrO- + 2H+ + 2e-

Second half reaction,

ClO4- ---> ClO3-

balance O and H,

ClO4- + 2H+ ---> ClO3- + H2O

add e-'s,

ClO4- + 2H+ + 2e- ---> ClO3- + H2O

Add both half reactions,

(b) Br- + ClO4- ---> BrO- + ClO3-

Is the net balanced equation

(c) In basic medium

Br- + ClO4- ---> BrO- + ClO3-

First half reaction

Br- ---> BrO-

balance O,

Br- + H2O --> BrO-

balance H,

Br- + H2O ---> BrO- + 2H+

Add OH-,

Br- + 2OH- ---> BrO- + H2O

add e-'s,

Br- + 2OH- ---> BrO- + H2O + 2e-

Second half reaction,

ClO4- ---> ClO3-

balance O and H,

ClO4- + 2H+ ---> ClO3- + H2O

Add OH-.

ClO4- + H2O ---> ClO3- + 2OH-

add e-'s,

ClO4- + H2O + 2e- ---> ClO3- + 2OH-

Add both half reactions,

Br- + ClO4- ---> BrO- + ClO3-

Is the net balanced equation

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects