An unknown compound contains $C, H$ and $O$ elements, it contains $48$ % $C$ and $4.0$ % $H$ by mass. The molar mass $200$ is determined in the lab. Find the molecular formula of this compound.

C_{2} H_{3} O_{2}

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C_{4} H_{6} O_{2}

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C_{4} H_{4} O_{3}

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C_{8} H_{3} O_{6}

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C_{8} H_{8} O_{6}

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Solution

The correct option is E $C_{8} H_{8} O_{6}$
100 g of compound will contain 48 g C, 4.0 g H and $100 - 48 - 4.0 = 48$ g O.
The atomic masses of C, H and O are 12, 1 and 16 g/mol respectively.
The number of moles of C $= \frac{4 g}{1 g / m o l} = 4 m o l$
The number of moles of H $= \frac{4 g}{1 g / m o l} = 4 m o l$
The number of moles of O $= \frac{48 g}{16 g / m o l} = 3 m o l$
$C : H : O = 4 : 4 : 3$
The empirical formula is $C_{4} H_{4} O_{3}$ .
Empirical formula mass $= 4 (12) + 4 (1) + 3 (16) = 100 g / m o l$
Molar mass = 200 g/mol
Molecular formula $= \frac{200}{100} \times C_{4} H_{4} O_{3} = C_{8} H_{8} O_{6}$

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An unknown compound contains C,H and O elements, it contains 48% C and 4.0% H by mass. The molar mass 200 is determined in the lab. Find the molecular formula of this compound.

An unknown compound contains $C, H$ and $O$ elements, it contains $48$ % $C$ and $4.0$ % $H$ by mass. The molar mass $200$ is determined in the lab. Find the molecular formula of this compound.