Question

Write a balanced half-reaction for the oxidation of aqueous hydrogen peroxide to gaseous oxygen in basic aqueous solution. Be sure to add physical state symbols where appropriate.

Answer 1

The balanced half-reaction for the oxidation of hydrogen peroxide (H2O2) to oxygen gas (O2) in basic solution is H2O2 (aq) → O2 (g) + 2H2O (l) + 2e-. This involves balancing the oxygen and hydrogen atoms as well as the charge by adding electrons.

Step-by-step explanation:

The balanced half-reaction for the oxidation of aqueous hydrogen peroxide to gaseous oxygen in a basic aqueous solution involves showing the changes in oxidation states and balancing the overall charges by adding electrons. Below is the balanced half-reaction:

H2O2 (aq) → O2 (g) + 2H2O (l) + 2e-

The equation demonstrates the transformation of hydrogen peroxide into oxygen gas and water, with hydrogen peroxide acting as the reducing agent, losing electrons in the process. The process involves balancing the number of oxygen and hydrogen atoms, and then balancing the overall charge by adding the appropriate number of electrons.

Steps to Balance the Half-Reaction in Basic Solution:

1. Write the skeletal equation for the reaction.
2. Balance the oxygens by adding water (H2O) to the opposite side of the reaction.
3. Balance the hydrogens by adding hydroxide ions (OH-) to the same side as the added water.
4. Combine H+ and OH- to yield additional water molecules, if H+ ions are present.
5. Balance the charge of the half-reaction by adding electrons.
6. Simplify by removing any redundant water molecules.