Please help me with the following questions (picture) and feel free to correct me if I have wrong answers with a brief explanation.Thank you Belan2) Consider the following unbalanced net ionic redox equation.CrO42- + SO32-→ Cr³* + SO42-(a) Name the oxidizing agent in this reaction.303, bacaust wen if itis not beingeduced, the other one CrO4) iobeing exidizod.2-obecauseen斗itis notbeing(b) Name the ion that is oxidized in this reaction.CrOyBalancedNetlonicEquition(c) Balance this net ionic redox equation in basic solution.BalancedNet

Oxidising and reducing agent can be identified in a reaction by considering their oxidation state.Answer: Given reaction is: CrO42- + SO32- → Cr3+ + SO42- We can write reduction half in terms of oxidation state of ion Cr6+ + 3e- → Cr3+ And oxidation: S4+ → S6+ + 2e- It means CrO42- getting reduced and SO32- getting oxidises. Answer: a) Since the oxidising agent is one which itself getting reduced, here reduction of CrO42- taking place, therefore oxidising agent is CrO42- b) Since SO32- having Sulphur in +4 oxidation state goes into SO42- where Sulphur is in +6 oxidation state => oxidation of SO32- is taking place in the reaction. c) Balanced reaction can be written by adding Hydroxide ion to balance in alkaline medium as: CrO42- + 3 SO32- + 5 H2O → 2 [Cr(OH)4]- + 3 SO42- + 2 OH- Thank you!