Calculate `EMF` of the following half cells `:`
`a. Pt, H_(2)(2 atm)|HCl(0.02M)" "E^(c-)=0V`
`b. Pt , Cl_(2)(10 atm)|HCl(0.1 M)" "E^(-c)=1.36V`

Explanation

To calculate the EMF (Electromotive Force) of the given half-cells, we will use the Nernst equation. The Nernst equation is given by:

\[ E = E^\circ - \frac{0.0591}{n} \log \left( \frac{[Ox]}{[Red]} \right) \]

Where:
- \( E \) is the cell potential (EMF)
- \( E^\circ \) is the standard cell potential
- \( n \) is the number of moles of electrons transferred in the reaction
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