Calculate the value of `E_("cell")` at 298 K for the following cell:
`Al//Al^(3+) (0.01M)"||" Sn^(2+) (0.015 M)//Sn`
`[E_(Al^(3+)//Al)^(Theta) = -1.66V and E_(Sn^(2+)//Sn)^(Theta) = -0.14V]`

Explanation

To calculate the value of \( E_{\text{cell}} \) at 298 K for the cell \( \text{Al} | \text{Al}^{3+} (0.01 \, \text{M}) || \text{Sn}^{2+} (0.015 \, \text{M}) | \text{Sn} \), we will follow these steps:

### Step 1: Identify the half-reactions
The half-reactions for the given cell are:
1. Oxidation (Anode):
\[ \text{Al} \rightarrow \text{Al}^{3+} + 3e^- \]
...