Question

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

Answer 1

The balanced half-reaction for the oxidation of liquid water to aqueous hydrogen peroxide in basic solution is OH(aq) + H(1) → H(aq) + 2 e.

Step-by-step explanation:

Half-Reaction for the Oxidation of Liquid Water to Hydrogen Peroxide

To write a balanced half-reaction for the oxidation of liquid water (H2O(l)) to hydrogen peroxide (H2O2(aq)) in a basic aqueous solution, we follow the half-reaction method. First, we identify the change in oxidation states and write the unbalanced half-reaction:

H2O(l) → H2O2(aq)

Next, we balance the oxygen atoms by adding water molecules to the appropriate side. Since the oxygen is already balanced, we move on to balance the hydrogen atoms by adding hydroxide ions (OH−) as it is a basic solution:

3 OH−(aq) + H2O(l) → H2O2(aq) + 2 OH−(aq) + 2 e−

Balance the charges by adding electrons to the reactants side. Now, we combine the hydroxide ions on the right and simplify:

3 OH−(aq) + H2O(l) → H2O2(aq) + 2 H2O(l) + 2 e−

We then simplify further to obtain the final balanced half-reaction:

OH−(aq) + H2O(l) → H2O2(aq) + 2 e−