I2(s)+ocl−(aq)→io−3(aq)+cl−(aq) (acidic solution)

Part-A The half reactionsof given redox reaction are shown below: 221O- OCCl All atoms are balanced except oxygens. Now, balance the oxygens by adding H2O Now, balance the hydrogens by adding H+ ions. Now, balance the charge in half reacti on. 1つ+6H,O-> 210 -+12H+ +10e Now balance the number of electronsandthen addthe twohalf reactions 1, +GE,°-> 210 -+ 12H+ +10e 50Cl-+ 10H+ +10e > 5Cl_ +5H2O Thus, the balancedreacti on isshown below. Part-B L is oxidised from 0 to 5. So, I, acts as reducing agent and OCl acts as oxidising agent

Part-C The half reactionsof given redox reaction are shown below: 2 3 All atoms are balanced except oxygens. Now, balance the oxygens by adding H2o 2N03--> N203 +3H20 Now, balance the hydrogens by adding H+ ions. Now, balance the charge in half reacti on. Now balance the number of electronsandthen addthe twohalf reactions 2 3 2 3 Thus, the balancedreacti on isshown below. As,03 + 2NO-+ 2H2O + 2H+-> 2H,AsO, + N203 Part-D Asis oxidised from + 3 to +5 and N isreduced from5 to +3 So, As,O3 acts as reducing agent and NO3 acts as oxidising agernt