Calculate `DeltaG^(@)` and log `K_(c)` for the following reaction at 298 K :
`2Al(s)+3Cu^(2+)(aq)rarr2Al^(3+)(aq)+3Cu(s)`
Given `E_(cell)^(@)`=2.02 V

Explanation

To solve the problem, we need to calculate the standard Gibbs free energy change (ΔG°) and the logarithm of the equilibrium constant (log Kc) for the given electrochemical reaction at 298 K.

### Step 1: Identify the Reaction and Calculate n (Number of Electrons Transferred)

The reaction is:
\[ 2 \text{Al}(s) + 3 \text{Cu}^{2+}(aq) \rightarrow 2 \text{Al}^{3+}(aq) + 3 \text{Cu}(s) \]

- **Oxidation half-reaction** (at the anode):
...