`CuSO_(4)(aq.)+Zn(s) to ZnSO_(4)+Cu uarr`

Options

A. For disproportionation reaction.
B. For comproportionation reaction.
C. For either intermolecular redox reaction or displacement reaction
D. For either thermal combination redox reaction or thermal decomposition redox reaction.

Answer

To solve the question regarding the reaction between CuSO₄ (aqueous) and Zn (solid), we can follow these steps:

### Step 1: Identify the Reactants and Products
The reactants in the reaction are Copper(II) sulfate (CuSO₄) in aqueous solution and Zinc (Zn) in solid form. The products of the reaction are Zinc sulfate (ZnSO₄) in aqueous solution and Copper (Cu) in solid form.

### Step 2: Write the Balanced Chemical Equation
The balanced chemical equation for the reaction is:
\[ \text{CuSO}_4(aq) + \text{Zn}(s) \rightarrow \text{ZnSO}_4(aq) + \text{Cu}(s) \]

### Step 3: Determine the Type of Reaction
This reaction is a single displacement (or single replacement) reaction. In this type of reaction, a more reactive metal (Zn) displaces a less reactive metal (Cu) from its compound (CuSO₄).

### Step 4: Analyze the Oxidation States
- In CuSO₄, Copper (Cu) has an oxidation state of +2.
- In Zn, the oxidation state is 0 (as it is in its elemental form).
- In ZnSO₄, Zinc (Zn) has an oxidation state of +2.
- In the product, Copper (Cu) is in its elemental form, so its oxidation state is 0.

### Step 5: Identify the Redox Changes
In this reaction:
- Zinc (Zn) is oxidized from 0 to +2 (loses electrons).
- Copper (Cu) is reduced from +2 to 0 (gains electrons).

### Step 6: Conclusion
This reaction is a redox reaction because there is a transfer of electrons between the reactants. It is also a displacement reaction because a more reactive metal (Zn) displaces a less reactive metal (Cu) from its compound.

### Final Answer
The reaction between CuSO₄ (aq) and Zn (s) is a **single displacement redox reaction**.

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