When $$0.01$$ mol of an organic compound containing $$60\%$$ carbon was burnt completely, $$4.4$$ g of CO$$_2$$ was produced. The molar mass of compound is ______ g mol$$^{-1}$$ (Nearest integer)

We need to find the molar mass of an organic compound containing 60% carbon, given that 0.01 mol produces 4.4 g of CO$$_2$$ on complete combustion.

Molar mass of CO$$_2$$ = 44 g/mol.

$$\text{Moles of CO}_2 = \frac{4.4}{44} = 0.1 \text{ mol}$$

Each mole of CO$$_2$$ contains 1 mole of carbon.

Moles of C = 0.1 mol from 0.01 mol of compound.

So each mole of compound contains $$\frac{0.1}{0.01} = 10$$ moles of carbon.

Mass of carbon per mole of compound = $$10 \times 12 = 120$$ g.

Since the compound is 60% carbon:

$$\frac{120}{M} = 0.60$$

$$M = \frac{120}{0.60} = 200 \text{ g/mol}$$

The correct answer is 200.