Solve this redox reaction and give the oxidation states of each element: CuSO4 + Zn = ZnSO4 + Cu

Steps to Solve

1. Identify the Oxidation States

We start by determining the oxidation states of each element in the reactants and products:

• In $CuSO_4$, copper (Cu) has an oxidation state of +2, and sulfate (SO4) has a charge of -2 overall.
• Zinc (Zn) starts with an oxidation state of 0 (as an elemental substance).
• In the product, zinc sulfate ($ZnSO_4$), zinc has an oxidation state of +2, while sulfate remains -2.
• The copper product can be elemental copper (Cu), which has an oxidation state of 0 when uncombined.

2. Write the Half-Reactions

Now, we will write the half-reactions for oxidation and reduction:

• Oxidation half-reaction: Zinc loses electrons (is oxidized): $$ Zn \rightarrow Zn^{2+} + 2e^- $$

• Reduction half-reaction: Copper gains electrons (is reduced): $$ Cu^{2+} + 2e^- \rightarrow Cu $$

3. Balance the Overall Reaction

Next, we combine the balanced half-reactions to write the overall balanced reaction. Since both half-reactions involve two electrons, we can add them directly:

$$ Zn + Cu^{2+} \rightarrow Zn^{2+} + Cu $$

4. Final Check of Balancing

Finally, ensure that the number of atoms and the charges are balanced:

• Reactants: 1 Zn and 1 Cu, with a total charge of 0 ($0$).
• Products: 1 Zn and 1 Cu, with a total charge of 0 ($+2 for Zn^{2+} and 0 for Cu$).

Both atoms and charges are balanced.