The `EMF` of the cell `:`
`Pt|Ce^(4+)(90%),Ce^(3+)(10%)|` Normal calomel electrode is `1.464 V` at `25^(@)C`. Find the value of equilibrium constant of the reaction `:`
`2Ce^(3+)+2H^(o+) rarr 2Ce^(4+)+H_(2)`
The electrode potential of the normal calomel electrode is `+0.28V`.

Explanation

To find the equilibrium constant \( K \) for the reaction:

\[ 2Ce^{3+} + 2H^+ \rightleftharpoons 2Ce^{4+} + H_2 \]

we will follow these steps:

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