dation number of N increases from -2 in to +2 in NO and the oxidation number of Cl decreases from + 5 in to -1 in . HENCE, in this reaction, is the reducing AGENT and is the oxidizing agent. i) Ion-electron method:The oxidation half equation is:The N ATOMS are balanced as:The oxidation number is balanced by adding 8 electrons as:The charge is balanced by adding 8 OH-ions as:The O atoms are balanced by adding 6H2O as:The reduction half equation is:The oxidation number is balanced by adding 6 electrons as:The charge is balanced by adding 6OH- ions as:The O atoms are balanced by adding 3H2O as:The balanced equation can be obtained by multiplying equation (i) with 3 and equation (ii) with 4 and then adding them as:ii) Oxidation number method:Total decrease in oxidation number of Total increase in oxidation number of On multiplying with 3 and with 4 to balance the increase and decrease in O and N, we get:The N and Cl atoms are balanced as:The O atoms are balanced by adding 6H2O as:This is the REQUIRED balanced equation.iii) In the above reaction is the reducing agent and is the oxidizing agent.