Problem: Balance each of the following redox reactions occurring in basic solution. a. H2O2(aq) + ClO2(aq) → ClO2-(aq) +O2(g)b. Al(s)+MnO4-(aq) → MnO2(s) + Al(OH)4-(aq)c. Cl2(g) → Cl−(aq)+ ClO−(aq)

🤓 Based on our data, we think this question is relevant for Professor Ruggles' class at VERMONT.

FREE Expert Solution

When balancing redox reactions under acidic conditions, we will follow the following steps.

Step 1: Separate the whole reaction into two half-reactions.

Step 2: Balance the non-hydrogen and non-oxygen elements first.

Step 3: Balance oxygen by adding H2O to the side that needs oxygen. (1 O: 1 H2O)

Step 4: Balance hydrogen by adding H+ to the side that needs hydrogen. (1 H: 1 H+)

Step 5: Balance the charges: add electrons to the more positive side (or less negative side).

Step 6: Balance electrons on the two half-reactions.

Step 7: Get the overall reaction by adding the two reactions.

When balancing under basic conditions, additional steps are required:

Step 8: Balance remaining H+ by adding an equal amount of OH ions to both sides.

Step 9: H+(aq) will combine with OH(aq) to form H2O(l).

Step 10: Cancel out common species.

a. H2O2(aq) + ClO2(aq) → ClO2-(aq) +O2(g)

(1-2): Separate and balance non-H and O atoms

H2O2(aq) →  O2(g)

ClO2(aq) → ClO2-(aq) 

(3): Add H2O

H2O2(aq) →  O2(g)

ClO2(aq) → ClO2-(aq) 

(4): Add H+

H2O2(aq) →  O2(g) + 2 H(aq) 

ClO2(aq) → ClO2-(aq) 

(5): Balance charges

H2O2(aq) →  O2(g) + 2 H(aq) + 2 e-

ClO2(aq) + 1 e- → ClO2-(aq) 

View Complete Written Solution
Problem Details

Balance each of the following redox reactions occurring in basic solution.

a. H2O2(aq) + ClO2(aq) → ClO2-(aq) +O2(g)

b. Al(s)+MnO4-(aq) → MnO2(s) + Al(OH)4-(aq)

c. Cl2(g) → Cl(aq)+ ClO(aq)