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## Homework Statement

When 1.11 g of a compound X is completely burnt,1.98 g of carbon dioxide and 0.81 g of water were formed. Which of the following could be X?

A. CH[tex]_{3}[/tex]CH[tex]_{2}[/tex]CH[tex]_{3}[/tex]

B. CH[tex]_{3}[/tex]CH[tex]_{2}[/tex]COOH

C.CH[tex]_{3}[/tex]COCH[tex]_{3}[/tex]

D.C[tex]_{6}[/tex]H[tex]_{5}[/tex]CH[tex]_{2}[/tex]OH

## The Attempt at a Solution

I tried

C[tex]_{x}[/tex]H[tex]_{y}[/tex] + {x+[tex]\frac{y}{4}[/tex]}O[tex]_{2}[/tex] [tex]\rightarrow[/tex]

XC0[tex]_{2}[/tex] + [tex]\frac{y}{2}[/tex]H[tex]_{2}[/tex]O

but how about the oxygen atom(s) within compound X?

How can I form a balanced equation for X containing O?

Sorry about the equations and formulae... can't get the subscripts in the right positions.

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