Calculate `E_(cell)^(@)` for the following reaction at 298 K:
`2AI(s) + 3Cu^(2+)(0.01M) to 2A1^(3+)(0.01M) + 3Cu(s)`
`"Given" : E_(cell) = 1.98V`
(b) Using the `E^(@)` values A and B, predict which is better for coating the surface of iron
`[E^(@)(Fe^(2+)//Fe) = -0.44V]` to prevent corrosion and why?
`"Given" : E^(@)(A^(2+)//A) = 2.37V : E^(@)(B^(2+) //B) = 0.14V`

Explanation

To solve the problem step by step, we will follow the outlined procedure to calculate \( E_{cell}^\circ \) for the given reaction and determine which metal is better for coating iron to prevent corrosion.

### Step 1: Write the Given Reaction
The reaction given is:
\[ 2 \text{Al}(s) + 3 \text{Cu}^{2+}(0.01M) \rightarrow 2 \text{Al}^{3+}(0.01M) + 3 \text{Cu}(s) \]

### Step 2: Identify the Standard Cell Potential Equation
The equation for the cell potential is given by:
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