2.In a redox reaction
Fe 2 O 3 + KNO 3 + KOH = K 2 FeO 4 + KNO 2 + H 2 O
find an oxidizing agent and a reducing agent, arrange the coefficients by any method (electronic or ion-electronic balance).
Now the oxidation number of Fe in reactant side is +3 but it increases to +6 on the product side so it oxidized hence it will behave as a Reducing agent.
The oxidation number of K in reactant side is +3 but it decreases to +1 on the product side so it reduced hence it will behave as a Oxidizing agent.
The balance chemical equation of the above is:
"Fe_2O_3+2KNO_3+2KOH \\longrightarrow 2K_2FeO_4+KNO_2 +H_20"