Separate this redox reaction into its component half-reactions.
O2 + 2Zn -->2ZnO
Is it already balanced as is? When I tried I got it to all cancel out.
I think it was balanced as you wrote it.
O2 + 4e==> 2O^2-
Zn ==> Zn2+ + 2e
Multiply equn 1 by 1 and eqn 2 by 2.
O2 + 4e ==> 2O^2-
2Zn ==> 2Zn^2+ + 4e and add
------------------
2Zn + O2 ==> 2ZnO
O2 == O^2-
Zn ==> Zn^2+
You can balance.
sorry which of this is the oxidation reagent and reduction reagent
To separate the given redox reaction into its component half-reactions, we need to identify the oxidation half-reaction and the reduction half-reaction.
In the given reaction:
O2 + 2Zn --> 2ZnO
1. Identify the atoms that undergo the oxidation and reduction. In this case, Zn is oxidized from Zn to ZnO, and O2 is reduced from O2 to ZnO.
2. Write the oxidation half-reaction, which represents the loss of electrons (oxidation):
Zn --> ZnO
3. Write the reduction half-reaction, which represents the gain of electrons (reduction):
O2 --> ZnO
So, the separate half-reactions for the given redox reaction are:
Oxidation half-reaction: Zn --> ZnO
Reduction half-reaction: O2 --> ZnO