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 need to determine the formula of sulfur based on the given data about the freezing point depression of a solution. Here’s a step-by-step solution:

### Step 1: Identify Given Data
- Mass of sulfur (solute), \( W_b = 25.6 \, \text{g} \)
- Mass of naphthalene (solvent), \( W_a = 1000 \, \text{g} \)
- Freezing point depression, \( \Delta T_f = 0.680 \, ^\circ C \)
- Freezing point depression constant for naphthalene, \( K_f = 6.8 \, \text{K kg}^{-1} \)

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