determine the empirical formula of a compound containing 48.38 grams of carbon, 8.12 grams of hydrogen, and 53.5 of oxygen. in an experiment, the molar mass of the compound was determined to be 180.15 g/mol. what is the molecular formula of the compound?

Question

Chemistry

Jay Compton

10 December, 10:23

determine the empirical formula of a compound containing 48.38 grams of carbon, 8.12 grams of hydrogen, and 53.5 of oxygen. in an experiment, the molar mass of the compound was determined to be 180.15 g/mol. what is the molecular formula of the compound?

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Answers (1)

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Luz · Answer 1

The molecular mass of this compound is 180 g/mol and could be Glucose

Explanation:

Step 1: Calculate moles

mole = mass / Molar mass

⇒ mole Carbon = 48.38 g/12 g/mol = 4.0317 moles

⇒ mole Hydrogen 8.12 g/1 g/mol = 8.12 moles

⇒ mole Oxygen 53.5 g/16 g/mol = 3.34375 moles

Step 2: Calculate the ratio

the smallest amount of moles is 3.34375 (oxygen), so we divide all by this number

⇒C = 4.0317/3.34375 = 1.206 ≈ 1

⇒H = 8.12.1 / 3.34375 = 2.425 ≈ 2

⇒O = 3.3437575/3.34375 = 1.00

Therefore; the empirical formula = CH2O

This has a molar mass of 30 g/mol

Now to find the molecular formula we divide 180.15 / 30 = 6

This means we have to multiply all numbers of elements by 6

The molecular formule = C6H12O6, which is glucose (or fructose, ...) and has a molar mass of 180g/mol