Balancing Redox Reactions
Balance each redox reaction in acidic solution using the half reaction method.
H2O2 + Cr2O72- → O2 + Cr3+
TeO32- + N2O4 → Te + NO3-
ReO4- +IO- → IO3- + Re
Balance each redox reaction in acidic solution using the half reaction method.
More Practice Balancing Redox Reactions in Acid and Basic Solution Balance the following redox reaction in both acidic and basic solution using the half reaction method outlined in Recitation 10, Part III. 3. Unbalanced: PbO2(s) + Mn2+(aq) → Pb2+ (aq) + MnO4- (aq) 4. Unbalanced: SO42-(aq) + Cr3+(aq) → SO2(g) + Cr2O72-(aq)
Balance the following redox equations by the half-reaction method: (a) Mn2+ + H2O2 → MnO2 + H2O (in basic solution) (b) Bi(OH)3 + SnO22− → SnO32− + Bi (in basic solution) (c) Cr2O72− + C2O42− → Cr3+ + CO2 (in acidic solution) (d) ClO3− + Cl− → Cl2 + ClO2 (in acidic solution) (e) Mn2+ + BiO3− → Bi3+ + MnO4− (in acidic solution)
Balance the folioing redox reactions via the 1/2 reaction method - Show all workCr2O72- +I- => Cr3 + IO3- ( In acidic solution)
Balance following redox reactions in acidic conditions using the half-reaction method a. Fe + Ag+ → Fe2+ + Ag b. I- + SO42- → H2S + I2 c. Cu + NO3- → Cu2+ + NO2 d. PbO₂ + CI- → Pb2+ + Cl₂
balance the following redox reactions in acidic solution by the half reaction method. Indicate which half reaction is for oxidation and which for reduction. b) Cr2O72- (aq) + CH(aq) > Cr*(aq) + Cl2(g) c) Au(s) + HNO3(aq) + HCl(aq) --> AuCl4- (aq) + NO(g) d) 103-(aq) + (aq) --> 13-(aq)
Show work please! Balance the following redox reaction in acidic solution using the half reaction method. Show each step clearly and show all work so that partial credit can be given if needed. 3.
D Question 29 1 pts Balance the following redox reaction using the half-reaction method in acidic solution. MnOd() + Fe2(04) Mn?"(aq) + Fea) What is the coefficient in front of Fe2in the balanced reaction? 01 O2 O 3 04 O 5 06 07 OB
5) Balance the following redox reactions. For each one, identify the reducin and the oxidizing agent. (acidic solution) a) Cr2O72- + NO2 = Cr3+ + NO3- (basic solution) b) H O2 + Cio2 = 02 + ClO2- (acidic solution) c) Mnox + VÕ2+ = Mn2+ + V(OH)4* d) AIS) + Noz = NH4+ + A102 (basic solution) e) 103- + 1 = 12 (acidic solution) f) SCN-+ Br03- = Br + SO42- + HCN (acidic solution)
4. Balance the redox reaction below using the half-reaction method. Fe +Cr,O,2Fe +Cr (acidic solution)
Part IV: Balancing Redox Reactions in Acidic and Basic Solution General rules for balancing redox reactions in acidic or basic solution: 1. Divide the redox reaction into two half-reactions. One that contains the element that gets Oxidized and one that contains the element that gets reduced. 2. Focusing on one half-reaction at a time, balance all non-H and non-0 atoms. 3. Balance the O atoms by adding water molecules to the side with too few oxygens 4. Balance the H...