Calculate the e.m.f of the following cell :
`Cd|Cd^(2+) (0.01 M) ||H^(+) (0.02 M) |Pt , H_(2) (0.8` atm)
Given : `E^(@) (Cd^(2+) |Cd) = -0.40V`

Explanation

To calculate the e.m.f. (electromotive force) of the given cell, we will follow these steps:

### Step 1: Identify the Anodic and Cathodic Reactions
- **Anodic Reaction (Oxidation)**: Cadmium is oxidized. The half-reaction is:
\[ \text{Cd} \rightarrow \text{Cd}^{2+} + 2e^- \]

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