We are being asked to balance the given redox reaction occurring in an acidic solution.
When balancing redox reactions under acidic conditions, we will follow the following steps.
Step 1. Separate the whole reaction into 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 reaction
Balance the redox reaction under basic condition:
H2O2(aq) + MnO4−(aq) ⟶ Mn2+(aq) + O2(g) (in acid)
Balance each of the following equations according to the half-reaction method:
(f) H2O2(aq) + MnO4−(aq) ⟶ Mn2+(aq) + O2(g) (in acid)
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Balancing Redox Reaction concept. You can view video lessons to learn Balancing Redox Reaction. Or if you need more Balancing Redox Reaction practice, you can also practice Balancing Redox Reaction practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Kadish's class at UH.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.