when a zinc is placed in a copper(ii)nitrate solution,the strip becomes coated with copper.write down the oxidation half reaction for the reaction that takes place.
To write the oxidation half-reaction for the reaction that takes place when a zinc strip is placed in a copper(II) nitrate solution, you need to understand the concept of oxidation and reduction.
In this reaction, zinc is being oxidized and loses electrons to form ions. Copper(II) ions are being reduced and gain those electrons to form copper metal.
The first step is to write the balanced chemical equation for the reaction:
Zn(s) + Cu(NO3)2(aq) → Cu(s) + Zn(NO3)2(aq)
Now, let's focus on the oxidation half-reaction. Since zinc loses electrons, it is being oxidized. The half-reaction equation can be determined by considering the change in oxidation state of zinc in the reaction:
Zn(s) → Zn2+(aq) + 2e-
In this equation, zinc (Zn) goes from an oxidation state of 0 to +2, indicating the loss of 2 electrons. That's why we add the 2e- on the right side, indicating the loss of 2 electrons.
So, the oxidation half-reaction for the reaction is:
Zn(s) → Zn2+(aq) + 2e-