A solution containing 2 g of a non-volatile solute in 20 g of water boils at 373.52 K. The molecular mass of the solute is ______ g mol$$^{-1}$$. (Nearest integer)
Given, water boils at 373 K, K$$_b$$ for water $$= 0.52$$ K kg mol$$^{-1}$$

To determine the molecular mass of a non-volatile solute from the elevation in boiling point, note that the solute mass is 2 g and the solvent mass is 20 g = 0.020 kg. The boiling point increase is $$\Delta T_b = 373.52 - 373 = 0.52$$ K, and the ebullioscopic constant is $$K_b = 0.52$$ K kg mol$$^{-1}$$.

Using the relation $$\Delta T_b = K_b \times m = K_b \times \frac{w_2}{M_2 \times w_1}$$ and substituting the values gives:

$$0.52 = 0.52 \times \frac{2}{M_2 \times 0.020}$$

Rearranging yields $$1 = \frac{2}{0.020 \times M_2} = \frac{100}{M_2}$$, so $$M_2 = 100$$ g/mol.

Therefore, the molecular mass of the solute is $$\boxed{100}$$ g mol$$^{-1}$$.