For galvanic cell,
`Ag|AgCl(s),CsCl(0.1M)||CsBr(10^(-3)M),AgBr(s)|Ag.`
Calculate the `EMF` generated and assign correct polarity to each electrode for spontaneous or exergonic process at `25^(@)C`.
Given `:. K_(sp)` of `AgCl=3.0xx10^(-10),K_(sp)` of `AgBr=4.0xx10^(-13)`.

Explanation

To solve the problem of calculating the EMF generated by the given galvanic cell and assigning the correct polarity to each electrode, we will follow these steps:

### Step 1: Determine the Concentration of Silver Ions (Ag⁺) at the Anode
The solubility product constant (Ksp) for AgCl is given as \(3.0 \times 10^{-10}\). The dissociation of AgCl can be represented as:
\[ \text{AgCl(s)} \rightleftharpoons \text{Ag}^+ + \text{Cl}^- \]
From the Ksp expression:
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