What is the empirical formula of a following compound if a sample contain 0.0130 mol $C$ $C$ , 0.0390 mol $H$ $H$ , and 0.0065 mol $O$ $O$ ?

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What is the empirical formula of a following compound if a sample contain 0.0130 mol $C$ $C$ , 0.0390 mol $H$ $H$ , and 0.0065 mol $O$ $O$ ?

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Answer 1 · 2016-03-07T07:59:28

We divide thru by the smallest molar quantity to write the empirical formula.

Explanation:

So the smallest molar quantity is that of oxgen, $C = \frac{0.0130 \cdot m o l}{0.0065 \cdot m o l}$ $C =(0.0130*mol)/(0.0065*mol)$ ; $H = \frac{0.0390 \cdot m o l}{0.0065 \cdot m o l}$ $H =(0.0390*mol)/(0.0065*mol)$ ; $O = \frac{0.0065 \cdot m o l}{0.0065 \cdot m o l}$ $O =(0.0065*mol)/(0.0065*mol)$ .

So $C_{n} H_{m} O_{p}$ $C_nH_mO_p$ $=$ $=$ $C_{2} H_{6} O$ $C_2H_6O$ .

So that's the empirical formula, the simplest whole number ratio that defines constituent atoms in a species. The molecular formula is some whole number multiple of the empirical formula.

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What is the empirical formula of a following compound if a sample contain 0.0130 mol $C$ $C$ , 0.0390 mol $H$ $H$ , and 0.0065 mol $O$ $O$ ?

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What is the empirical formula of a following compound if a sample contain 0.0130 mol CC, 0.0390 mol HH, and 0.0065 mol OO?

1 Answer

Explanation:

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What is the empirical formula of a following compound if a sample contain 0.0130 mol $C$ $C$ , 0.0390 mol $H$ $H$ , and 0.0065 mol $O$ $O$ ?