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 determine which reaction is likely to proceed when an iron rod is immersed in a solution containing `1.0 M NiSO4` and `1.0 M ZnSO4`, we need to analyze the standard reduction potentials (SRP) given for the half-reactions:

1. `E_(Zn^(2+)|Zn)^(0)` = -0.76 V
2. `E_(Fe^(2+)|Fe)^(0)` = -0.44 V
3. `E_(Ni^(2+)|Ni)^(0)` = -0.25 V

### Step 1: Identify the reducing and oxidizing agents
- The standard reduction potential indicates the tendency of a species to gain electrons (be reduced). A more negative value means a weaker tendency to be reduced, making it a better reducing agent.
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