A solution containing `25.6 g` of sulphur, dissolved in `1000 g` of naphthalene whose melting point is `80.1^(@)C` gave a freezing point lowering of `0.680^(@)C`. Calculate the formula of sulphur (`K_(f)` for napthalene =`6.8 K m^(-1)`)

Explanation

To solve the problem, we will follow these steps:

### Step 1: Understand the relationship between freezing point depression and molality.
The formula for freezing point depression is given by:
\[ \Delta T_f = K_f \cdot m \]
where:
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