A solution was prepared by dissolving `6.0 g` an organic compound in `100 g` of water. Calculate the osmotic pressure of this solution at `298 K`,when the boiling point of the Solution is `100.2^(@)C`. (`K_(b)` for water =`0.52 K m^(-1)`), R=0.082 L atm `K^(_1) mol^(-1)`)

Explanation

To calculate the osmotic pressure of the solution, we will follow these steps:

### Step 1: Calculate the elevation in boiling point (ΔTb)
The boiling point of the solution is given as \(100.2^\circ C\) and the boiling point of pure water is \(100^\circ C\).

\[ \Delta T_b = T_{\text{solution}} - T_{\text{water}} = 100.2^\circ C - 100^\circ C = 0.2^\circ C \]
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