Balance the following redox reaction: H2O2(aq) + MnO4-(aq) ↔ O2(g) + Mn2+(aq)
Increase in oxidation number (O.N) is known as oxidation. Decrease in oxidation number is known as reduction.
Oxidation half reaction :-
H2O2 (aq) ------> O2(g) + 2H^+(aq) + 2e^- ---------(1)
Reduction half reaction :-
MnO4^-(aq) +8H^+(aq) + 5e^- -----> Mn^2+(aq) + 4H2O(l) ----(2)
Multiply (1) by 5 and (2) by 2 and then add it
5H2O2(aq) -----> 5O2(g) + 10H^+(aq) + 10e^-
2MnO4^-(aq) + 16H^+(aq) + 10e^- ----> 2Mn^2+(aq) + 8H2O(l)
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5H2O2(aq) + 2MnO4^-(aq) + 6H^+(aq) ----> 5O2(g) + 2Mn^2+(aq) + 8H2O(l)
This is balanced equation in acidic medium.
Balance the following redox reaction: H2O2(aq) + MnO4-(aq) ↔ O2(g) + Mn2+(aq)
Complete and balance the following reactions: H2O2 + MnO4- ----> O2 + Mn2+ (acid solution) H2O2 + MnO4- ----> O2 + Mn2+ (base solution) * please clearly explain
MnO4 (aq) + H2 C2O4(aq)Mn2+(aq) + CO2(g) 2. What element is being reduced in the following redox reaction? MnO4 (aq) + H2C2O4(aq) Mn2+(aq) + CO2(g)
Balance the following Redox reaction, which occurs in Acidic solution: Mn2+ (aq) MnO4 (aq) + H,C204(aq) + CO2(aq)
Use the half-reaction method to balance each redox reaction occurring in acidic aqueous solution. Cl−(aq)+MnO4−(aq)→Cl2(g)+Mn2+(aq) Express your answer as a chemical equation. Identify all of the phases in your answer.
2 MnO4 (aq) + 5 H2O2(aq) + 6 H(aq) → 5 O2(aq) + 2 Mn2+ (aq) + 8 H20(1) completely oxidize 25.0 mL of a H2O2 solution, calculate the molarity of the H20, solution
1. Balance the following reaction in acidic solution. I-(aq) + MnO4-(aq) Mn2+(aq) + I2(s) 2. Write a balanced net ionic equation for the following reaction in basic solution using both methods for balancing a redox reaction: Zn(s) + NO3-(aq) à NH3 (aq) + Zn(OH)42- (aq) 3. Write a balanced net ionic equation for the following reaction in basic solution using both methods for balancing a redox reaction: MnO4-(aq) + C2H5OH(aq) à Mn2+(aq) + HC2H3O2 (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)
2. Balance the following redox equation in a acidic solution: MnO4 (aq) + As«O6(s) → AsO4 (aq) + Mn2+(aq)
After balancing the following redox reaction, what is the coefficient of H+? MnO4-(aq) + SO2(g) + H2O(l) → Mn2+(aq) + SO42-(aq) + H+ (aq)
Balance the following ionic equation for a redox reaction, using whole number coefficients. MnO4-(aq)+SO2−3(aq)+H3O+(aq)⟶Mn2+(aq)+SO2−4(aq)+H2O(l) In the balanced equation, what is the coefficient for H2O? (this is the exact equation in the textbook)