Balance the reactions below on paper and upload to the assignment. SHOW ALL WORK! Balance the following reaction in acidic solution: Cr,0,2 (aq) + I' (aq)Cr3+ (aq) +12 (s) +Cr* (aq) +l2 (s) Balance the following reaction in basic solution: MnO4 (aq) +C2O42 (aq) MnO2(s) +CO32 (aq) Previous Next unit 3 exam.pdf Problem Set 3...pdf problem set 2.pdf MacBook Air 20 F3 F2 F4 F5 F6 F7 F8 F9 23 & 4 9. E D н J B くo TI

A. Balance the following redox reactions using the half-reaction method. B. Identify the oxidizing agent and the reducing agent. 1. Zn(s) + Fe²+ (aq) → Zn²+ (aq) + Fe (s) 2+ Zn(s) → Zn² +2e- oxidiation haut reaction (aq) 2+ 20+ Fe (an) → Fe (5) Reducation haut reaction (94) - Bris) Reducing agent (S) Fe 2+ oxidizing agent 2. (Balance this reaction In Acidic Solution):

Balance the following reaction in basic solution. Fill in the coefficients for the balanced overall equation. Al(s) + CrO (ag) → Al(OH)3(s) + Cr(OH), (aq) → 4 4. --v H0+ -- v Al + -v " →-v Al(OH), + -- v Cr(OH), + --v OH CrO, Cr(OH), + -- v OH 4 3.

Balance the following redox reaction in acidic solution. Fe²+(aq)+MnO2(s) Fe3+ (aq)+Mn2+ (aq) Fe2+ (aq) + MnO2 (s) - - Fe3+ (aq) + Mn2+(aq) ローロ ē ☑

Determine the Oxidizing and Reducing Agent in the reactions below:3 Cl2(g) + 2 Fe(s) → 6 Cl– (aq) + 2 Fe3+(aq)Oxidizing Agent:Reducing Agent:Zn2+(aq) + NH4+(aq) → Zn(s) + NO3– (aq) Oxidizing Agent:Reducing Agent:

Balance the equation below assuming the reaction occurs in a basic solution.  SO3²-(aq)+Cu(OH2(s)=SO4²-(aq)+Cu(OH)(s)

The hydroperoxide ion, HO2–(aq), reacts with permanganate ion, MnO4–(aq) to produce MnO2(s) and oxygen gas. Balance the equation for the oxidation of hydroperoxide ion to O2(g) by permanganate ion in a basic solution.

Balance the equation for the following redox reaction in an acidic solution: Show the half-reactions for oxidation and reduction. Show your work and oxidation numbers. -2 Cr₂0₁² (aq) + H₂SO3(aq) → Cr3 + HSO4 (aq) (aq)