The cell consists of three compartments separated by porous barriers. The first contains a cobalt electrode in 5.00 L of 0.100 M cobalt (II) nitrate, the second contains 5.00 L of 0.100M `AgNO_(3)`. Assuming that the current within the cell is carried equally by the positive and negative ions, tabulate the concentrations of ions of each type in each compartment of the cell after the passage of 0.100 mole electrons.
given `Co^(2+)+2e^(-)toCo" "E^(0)=-0.28V`
`Ag^(+)+e^(-)toAg" "E^(0)=0.80V`
Spontaneous reaction is: `2Ag^(+)+Co^(2+)+2Ag" "1.08V`

Explanation

To solve the problem, we need to determine the concentrations of ions in each compartment after the passage of 0.100 moles of electrons. We will analyze the reactions occurring at the cobalt and silver electrodes and then calculate the resulting concentrations of ions.

### Step-by-Step Solution:

1. **Identify the Reactions**:
- At the cobalt electrode:
\[
\text{Co}^{2+} + 2e^- \rightarrow \text{Co} \quad (E^{0} = -0.28 \, \text{V})
...