The empirical formula and molecular mass of a compound are ${\mathrm{CH}}_2\mathrm{O}$ and 180 g, respectively. The molecular formula of the compound is:
1. C₉H₁₈O₉
2. CH₂O
3. C₆H₁₂O₆
4. C₂H₄O₂

The molar mass of naturally occurring Argon isotopes is: 

On complete combustion, 44 g of a sample of a compound gives 88 g CO₂ and 36 g of H₂O. The molecular formula of the compound may be:

1.  ${\mathrm{C}}_4{\mathrm{H}}_6$ $$

2.  ${\mathrm{C}}_2{\mathrm{H}}_6\mathrm{O}$ $$

3.  ${\mathrm{C}}_2{\mathrm{H}}_4\mathrm{O}$

4.  ${\mathrm{C}}_3{\mathrm{H}}_6\mathrm{O}$

An organic compound contains carbon, hydrogen, and oxygen. If elemental analysis reveals 38.71% carbon and 9.67% hydrogen, which of the following is its empirical formula?