Question

Write a balanced half reaction for the oxidation of aqueous hydrazine (N₂H₄) to gaseous nitrogen (N₂) in acidic aqueous solution. Be sure to add physical state symbols where appropriate.

Answer 1

The balanced half reaction for the oxidation of aqueous hydrazine (N2H4) to gaseous nitrogen (N2) in acidic aqueous solution is N2H4(aq) -> N2(g) + 4H+(aq) + 4e-.

Step-by-step explanation:

The balanced half reaction for the oxidation of aqueous hydrazine (N2H4) to gaseous nitrogen (N2) in acidic aqueous solution is as follows:

N2H4(aq) → N2(g) + 4H+(aq) + 4e-

Step-by-step explanation:

1. The oxidation half-reaction shows the loss of electrons by hydrazine and the formation of products. In this case, hydrazine is oxidized to gaseous nitrogen.
2. The balanced equation includes the physical states of the reactants and products, with (aq) representing aqueous solution and (g) representing gas.
3. The presence of 4H+(aq) + 4e- on the product side balances the charge in the reaction.