A graph is plotted between `E_(cell)` and `log .([Zn^(2+)])/([Cu^(2+)])` . The curve is linear with intercept on `E_(cell)` axis equals to `1.10V`. Calculate `E_(cell)` for the cell.
`Zn(s)||Zn^(2+)(0.1M)||Cu^(2+)(0.01M)|Cu`

Explanation

To solve the problem, we will follow these steps:

### Step 1: Understand the cell representation
The cell representation given is:
\[ \text{Zn(s)} || \text{Zn}^{2+}(0.1M) || \text{Cu}^{2+}(0.01M) | \text{Cu(s)} \]
This indicates that zinc is the anode and copper is the cathode.

### Step 2: Write the half-reactions
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