Question

A compound containing 5.9265% hydrogen and 94.0735% oxygen has a molar mass of 34.01468 g/mol. Determine...

A compound containing 5.9265% hydrogen and 94.0735% oxygen has a molar mass of 34.01468 g/mol. Determine the empirical and molecular formula for this compound.

(Please show all formulas and work. Thank You)

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Homework Answers

Answer #1

Molecular formula H2O2

Empirical formula HO

Explanation

Mass of Hydrogen = (5.9265/100)× 34.01468g = 2.01588g

Mass of Oxygen = ( 94.0735/100) × 34.01468g = 31.9988g

Molar mass of Hydrogen = 1.00794g/mol

No of mole of Hydrogen = 2.01588g/1.00794(g/mol) = 2

Molar mass of Oxygen = 15.999g/mol

No of mole of Oxygen = 31.9988g/15.999g/mol = 2

Therefore

Molecular formula = H2O2

Empirical formula

ratio of Hydrogen = No of mole of Oxygen /No of mole of Hydrogen = 2/2 =1

ratio of Oxygen = No of mole of Oxygen / No of mole of Hydrogen = 2/2 =1

Therefore,

Empirical formula = HO

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