For Tube 4, you are given multiple choice questions and asked to choose the correct oxidation and reduction reaction and then the overall balanced equation. You should use this space to work on these equations. OX: HSO₂ (aq) → SO² (aq) RED: MnO4 → MnO₂ For Tube 5 you'll be given the oxidation reaction and asked to provide the overall balanced equation the reduction reaction is not given. If you've done your work in Table 1 and 2 above, you know what the reduction product is in Tube 5. The reactant is the same in all of the tubes (MnO4) so all you'll have to do is complete the mass and charge balance for this reaction in acidic solution to give you a correctly balanced reduction reaction along with the oxidation half- reaction. Then proceed with completing the overall reaction. You are required to upload this data sheet to show your work for this question. Red: MnO +8H* +5€→ Mn²+ 4 H₂O V compounds....asking about which is best oxidizing agent and which is best reducing agent Ox agent-stuff is reduced---need high ox # Red agent-stuff oxidized-low ox # [VO(H₂O)s]* vo solve for V ox # I have provided two unbalanced half-reactions for this process. You should understand how I knew it was MnO4 in the product for the reduction reaction. To reinforce the video from CH 16 about balancing in basic solution, try completing the balance of these in acidic solution first, then in basic. Hints: balance O first in the Ox equation by adding the appropriate # of H₂O- then add the appropriate # of H* (don't forget the H in HSO3). Then, after you've checked your mass balance, add up charges on both sides (remember the + charge in H* multiples by all the stoichiometric coefficient on H¹). The Red equation only needs charge balance, so that's easy! Ox: HSO₂ (aq) Red: MnO4 (aq) → SO4²- (aq) → MnO4² (aq) Overall balanced redox reaction in acidic solution: 2MnO4 (aq) +HSO³° (aq)+H₂O(l) → 2MnO4² (aq) +SO4²- (aq)+3H* (aq) Overall balanced redox reaction in basic solution