Calculate the potential of the following cell `Sn^(4+)(1.5M)+ZnrarrSn^(2+)(0.5M)+zn^(2+)(2M)`.
`"Given : "E_(Sn^(4+)//Sn^(2+))^(@)0.13V, E_(Zn^(2+)//Zn)^(@)=-0.76V`
Will the cell potential `uarr` or `darr` if the concentration of Sn4+ is increased ?

Explanation

To calculate the potential of the given electrochemical cell, we will use the Nernst equation. The cell reaction involves the reduction of \( \text{Sn}^{4+} \) to \( \text{Sn}^{2+} \) and the oxidation of \( \text{Zn} \) to \( \text{Zn}^{2+} \).

### Step-by-step Solution:

1. **Identify the half-reactions and their standard potentials:**
- The reduction half-reaction for tin:
\[
\text{Sn}^{4+} + 2e^- \rightarrow \text{Sn}^{2+} \quad E^\circ = 0.13 \, \text{V}
...