This is an oxidation-reduction (redox) reaction:
12 NV + 12 e- → 12 NIV (reduction)
6 O-II - 12 e- → 6 O0 (oxidation)
Cr(NO3)3 is an oxidizing agent, Cr(NO3)3 is a reducing agent.
Word equation
chromium nitrate → oxygen + nitrogen dioxide + chromium(III) oxide
Input interpretation
CrN3O9 → O2 + NO2 + Cr2O3
chromium nitrate oxygen nitrogen dioxide chromium(III) oxide
Balanced equation
Balance the chemical equation algebraically:
CrN3O9 → O2 + NO2 + Cr2O3
Add stoichiometric coefficients, c, to the reactants and products:
c1CrN3O9 → c2O2 + c3NO2 + c4Cr2O3
Set the number of atoms in the reactants equal to the number of atoms in the products for Cr, N and O:
Cr: c1 = 2c4
N: 3c1 = c3
O: 9c1 = 2c2 + 2c3 + 3c4
Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c4 = 1 and solve the system of equations for the remaining coefficients:
c1 = 2 c2= 3/2
c3=6 c4=1
Multiply by the least common denominator, 2, to eliminate fractional coefficients:
c1 = 4 c2=3
c3 = 12 c4 = 2
Substitute the coefficients into the chemical reaction to obtain the balanced equation:
Answer:
CrN3O9 → O2 + NO2 + Cr2O3
