Calculate the vapour pressure of 0.6% aqueous solution of a non-volatile, non-electrolyte solute, urea `(NH_2CONH_2)` at `25^@C`. The vapour pressure of pure water at `25^@C` is 24 mm Hg. Take densities to be 1 g `ml^(-1)` and assume ideal behaviour of the solution. Gas constant, R = 0.082 L atm. `mol^(-1)K^(-1)`.

Explanation

To calculate the vapor pressure of a 0.6% aqueous solution of urea at 25°C, we can follow these steps:

### Step 1: Understand the Given Data
- Vapor pressure of pure water, \( P_0 = 24 \, \text{mm Hg} \)
- Concentration of urea solution = 0.6% (w/v)
- Density of solution = 1 g/mL
- Molar mass of urea, \( \text{NH}_2\text{CONH}_2 \) = 60 g/mol (calculated as \( 14 + 1 + 12 + 16 = 60 \))
- Molar mass of water = 18 g/mol
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