Calculate `Delta_(r)G^(@)` and log `K_(c)` for the following reaction at 298 K.
`2Cr_((s))+Cd_((aq))^(3+)+33Cd_((s)){Given :E^(@)""_(Cell")=+0.34V,IF=96500Cmol^(-1)]`

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 reaction at 298 K.

### Step-by-Step Solution:

1. **Identify the Reaction and Determine n**:
The reaction given is:
\[
2 \text{Cr}_{(s)} + \text{Cd}^{3+}_{(aq)} \rightarrow 3 \text{Cd}_{(s)} + 2 \text{Cr}^{3+}_{(aq)}
...