A compound consists of 65.45% C, 5.492% H, and 29.06% O on a mass basis and has a molar mass of 110 g/mol. Determine the molecular formula of the compound.

Question

Chemistry

Lion

13 May, 13:51

A compound consists of 65.45% C, 5.492% H, and 29.06% O on a mass basis and has a molar mass of 110 g/mol. Determine the molecular formula of the compound.

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Answers (1)

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Aniya Stone · Answer 1

The molecular formula is C6H6O2

Explanation:

Step 1: Data given

Suppose the mass of the compound = 100 grams

The compound has:

65.45 % C = 65.45 grams

5.492 % H = 5.49 grams

29.06 % O = 29.06 grams

Molar mass C = 12.01 g/mol

Molar mass H = 1.01 g/mol

Molar mass O = 16.00 g/mol

Molar mass = 110 g/mol

Step 2: Calculate moles

Moles = mass / molar mass

Moles C = 65.45 grams / 12.01 g/mol

Moles C = 5.450 moles

Moles H = 5.49 grams / 1.01 g/mol

Moles H = 5.44 moles

Moles O = 29.06 grams / 16.00 g/mol

Moles O = 1.816 moles

Step 3: Calculate mol ratio

We divide by the smallest amount of moles

Moles C = 5.450 moles / 1.816 = 3

Moles H = 5.44 moles / 1.816 = 3

Moles O = 1.816/1.816 = 1

The empirical formula is C3H3O

The molar mass of this formula is 55 g/mol

We have to multiply the empirical formula by n

n = 110/55 = 2

2 * (C3H3O) = C6H6O2

The molecular formula is C6H6O2