The e.m.f. (`E^(0)` )of the following cells are
`Ag| Ag^(+)(1M) | | Cu^(2+)(1M) | Cu, E^(0) = -0.46V`,`Zn|Zn^(2+)(1M)| | Cu^(2+)(1M) | Cu : E^(0) = +1.10V`
Calculate the e.m.f. of the cell `Zn | Zn^(2+)(1M) | | Ag^(+)(1M) | Ag`

Explanation

To calculate the e.m.f. of the cell `Zn | Zn^(2+)(1M) | | Ag^(+)(1M) | Ag`, we will use the standard reduction potentials of the half-reactions involved. The e.m.f. of a cell can be calculated using the formula:

\[ E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \]

### Step 1: Identify the half-reactions and their standard reduction potentials

From the given data:
1. For the cell `Ag | Ag^(+)(1M) | | Cu^(2+)(1M) | Cu`, the standard e.m.f. is \( E^\circ = -0.46 \, V \).
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