$$\therefore\,\,\,$$ The ratio of no of atoms of C and H in one molecule of C_x H_y O_z = 1 : 2

$$\therefore\,\,\,$$ y = 2x

In one molecule of C_x H_y O_z compound contain z atoms of oxygen.

According to the question, no of atoms of oxygen required to burn C_xH_y completely should be twice of z atoms of oxygen.

C_xH_y + (x + $${y \over 4}$$) O₂ $$ \to $$ HCO₂ + $${y \over 2}$$ H₂O

No. of O₂ molecules required = (x + $${y \over 4}$$)

$$\therefore\,\,\,$$ No. of O atoms required = 2 (x + $${y \over 4}$$)

According to question,

$$2\left( {x + {y \over 4}} \right) = 2z$$

$$ \Rightarrow \,\,\,2\left( {x + {{2x} \over 4}} \right) = 2z\,\,\,$$ [ Putting y = 2x ]

$$ \Rightarrow \,\,\,\,{{3x} \over 2} = z$$

$$\therefore\,\,\,$$ x : y : z

= x : 2x : $${{3x} \over 2}$$

= 2 : 4 : 3

$$\therefore\,\,\,$$ Empirical formula = C₂H₄O₃