Question

A compound is 75.46% Carbon, 4.43% hydrogen and 20.10% Oxygen by mass. it has a molecular weight of 318.31g/mol. what is the molecular formula of the compound?
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Answer 1

Answer:

No.of moles of C is , n = mass/molar mass = 75.46 g / 12 (g/mol) = 6.3 moles No.of moles of H is , n' = mass/molar mass = 4.43 g / 1.0(g/mol) = 4.43 moles No.of moles of O is , n'' = mass/molar mass = 20.10 g / 16(g/mol) =1.25 moles Ratio to the no.of moles of C,H& O is 6.3 : 4.43 : 1.25 In the simple integer ratio is ( 6.3/1.25) : ( 4.43/1.25) : (1.25/1.25) 5.04 :3.5 : 1

Explanation:

Answer 2

We have that the Molecular Formula is

$C_{20}H_14O_4$

From the Question we are told that

75.46% Carbon

4.43% hydrogen

20.10% Oxygen

molecular weight of $318.31g/mol.$

Generally

Moles of Hydrogen

$M_c=\frac{75.46}{12}\\\\M_C=6.28\\\\M_C=\frac{6.28}{1.256}\\\\M_C=5$

$M_C=\frac{4.43}{1}\\\\M_C=4.43\\\\M_C=4.43/1.256\\\\M_C=3.5$

$M_c=\frac{20.10}{16}\\\\M_C=1.256/1.256\\\\M_C=1$

Therefore

Empirical  Formula

$C_{10}H_7O_2$

Where

$n=\frac{318.31g}{159}$

n=2

Molecular Formula

$C_{20}H_14O_4$

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