With the previous determined multiplier, place them as coefficients in front of oxidizing and reducing species to balance the oxidized and reduced atoms within. In this case, the coefficients of Cr₂O₇^2-, HNO₂, Cr³⁺ and NO₃^- in the equation are determined by the bracket information, which indicates that two Cr atoms undergo an oxidation change for every three N atoms that change. Therefore, place 2 (1x2) in front of Cr³⁺ and place 3 in front of both HNO₂ and NO₃^-.

In a disproportionation reaction, the coefficients of the substance involved in oxidation and reduction can be combined into one. In the case below, 3 (2+1) for HNO₂ (one of them undergoes oxidation and two of them undergo reduction), 1 for HNO₃ and 2 for NO.