when a zinc strip is placed in a copper nitrate solution, the strip becomes coated with copper. write down the oxidation half-reaction for the reaction that takes place.
Zn ==> Zn^+2 + 2e
cathode: Cu^2+ + 2e = Cu
anode: Zn - 2e = Zn^2+
Zn + Cu(NO3)2 = Zn(NO3)2 + Cu
Zn-zn'2+2e
To write down the oxidation half-reaction for the given reaction, we need to identify the changes that occur to the reactants. In this case, the zinc strip loses electrons and gets oxidized while copper ions in the copper nitrate solution gain those electrons and are reduced.
Here's how you can determine the oxidation half-reaction:
1. Identify the reactant getting oxidized: In this case, it is the zinc strip.
2. Write the oxidation state of the atoms involved:
- Zinc (Zn) has an oxidation state of 0 since it is an element on its own.
- Copper (Cu) in the copper nitrate solution has an oxidation state of +2 because it forms Cu2+ ions.
3. Determine the changes in oxidation states:
- Zinc goes from an oxidation state of 0 to a charge of +2. It loses two electrons to achieve the +2 charge.
- Copper goes from an oxidation state of +2 to zero as it receives the two electrons from zinc.
4. Write the balanced half-reaction:
- The oxidation half-reaction is written as: Zn -> Zn2+ + 2e-
So, the oxidation half-reaction for the given reaction is:
Zn -> Zn2+ + 2e-