**Step 1: **The reaction would be:

**C**_{x}**H _{y}O_{z} + O_{2} → CO_{2} + H_{2}O**

The mass of C and H:

$\mathbf{Mass}\mathbf{}\mathbf{C}\mathbf{=}\mathbf{4.401}\overline{)\mathbf{g}\mathbf{}{\mathbf{CO}}_{\mathbf{2}}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{CO}}_{\mathbf{2}}}}{\mathbf{44}\mathbf{.}\mathbf{01}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{CO}}_{\mathbf{2}}}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}\mathbf{C}}}{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{CO}}_{\mathbf{2}}}}\mathbf{\times}\frac{\mathbf{12}\mathbf{.}\mathbf{01}\mathbf{}\mathbf{g}\mathbf{}\mathbf{C}}{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}\mathbf{C}}}$

The compound dioxane, which is used as a solvent in various industrial processes, is composed of C, H, and O atoms. Combustion of a 2.203-g sample of this compound produces 4.401 g CO_{2} and 1.802 g H_{2}O. A separate experiment shows that it has a molar mass of 88.1 g/mol. Which of the following is the correct molecular formula for dioxane

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