Calculate the e.m.f. of a cell in which the following reactions take place at different electrodes.
`Zn^(2+) +2e^(-) to Zn, E^(Theta)= -0.76V " "...(i)`
`Ag^(+)+e^(-) to Ag, E^(Theta)=0.79V" "...(ii)`

Explanation

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

### Step 1: Identify the half-reactions and their standard electrode potentials.
We have two half-reactions:
1. **Zinc Reaction**:
\[ \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn}, \quad E^\Theta = -0.76 \, \text{V} \quad \text{(i)} \]
...