1. Find mass of carbon from $CO_2$

On complete combustion, all carbon in the compound becomes $CO_2$.

Given: $330\text{ g of }CO_2$

Molar mass of $CO_2 = 44$ g/mol, and each 44 g of $CO_2$ contains 12 g of carbon.

So, mass of carbon is: $\text{Mass of C} = 330\times \frac{12}{44} = 330\times \frac{3}{11} = 90\text{ g}$

2. Find mass of hydrogen from $H_2O$

All hydrogen in the compound becomes water.

Given: $270\text{ g of }H_2O$

Molar mass of $H_2O = 18$ g/mol, and each 18 g of $H_2O$ contains 2 g of hydrogen.

So, mass of hydrogen is: $\text{Mass of H} = 270\times \frac{2}{18} = 270\times \frac{1}{9} = 30\text{ g}$

3. Check total mass

$90 + 30 = 120\text{ g}$

This matches the given mass of the compound, so the calculation is consistent.

4. Calculate percentage composition

Percentage of carbon: $\%C = \frac{90}{120}\times 100 = 75\%$

Percentage of hydrogen: $\%H = \frac{30}{120}\times 100 = 25\%$

5. Match with options

The percentages of carbon and hydrogen respectively are: $75\% \text{ and } 25\%$

So the correct option is D.