An iron rod is immersed in a solution containing `1.0 M NiSO_(4)` and `1.0 M ZnSO_(4)` Predict giving reasons which of the following reactions is likely to proceed ?
(i) Fe reduces `Zn^(2+)` ions,
(ii) Iron reduces `Ni^(2+)` ions.
Given : `E_(Zn^(2+)| Zn )^(0)` = -0.76 volt and ,`E_(Fe^(2+)|Fe)^(0)` = -0.44 volt and `E_(Ni^(2+)|Ni)^(0)`= -0.25 V

Explanation

To solve the problem, we need to analyze the two reactions involving the iron rod in the presence of `1.0 M NiSO4` and `1.0 M ZnSO4`. We will determine which reaction is likely to proceed based on the standard reduction potentials provided.

### Step 1: Identify the Reactions

1. **Reaction 1**: Fe reduces `Zn^(2+)` ions.
- The reaction can be written as:
\[
\text{Fe} + \text{Zn}^{2+} \rightarrow \text{Fe}^{2+} + \text{Zn}
...