Addison-Wesley CHEMISTRY Balancing Redox equations (pg. 607-8) Step 4: Make the total increase in oxidation number equal to the total decrease in oxidation number by using appropriate coefficients. Practice problem 10b. KClO (s)==>KCl(aq) + O2(g) When I did step 4 of this equation, I was unable to understand why and how the fraction 3/2 is put in front of the oxygen gas in the product side. And also why oxygen is chosen from all the other compounds to place the coefficient infront. I would like this point clarified because its been hindering me of comprehending and solving similar equations.