A mixture which contains `0.550 g` of camphor and `0.090 g` of an organic solute melts at `161^(@)C`. The solute contains `93.75%C` and `6.25%` H by weight.What is the molecular formula of compound? `K_(f)` for camphor is `37.5^(@)C "mol"^(-1) kg`. The melting point of camphor is `209^(@)C`.

Explanation

To determine the molecular formula of the organic solute, we will follow these steps:

### Step 1: Calculate the Depression in Freezing Point (ΔTf)
The melting point of pure camphor is given as \( 209^\circ C \) and the melting point of the mixture is \( 161^\circ C \).

\[ \Delta T_f = T_f^{\text{pure}} - T_f^{\text{mixture}} = 209^\circ C - 161^\circ C = 48^\circ C \]
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