Question

What is the molecular formula for a compound that is 46.16% carbon, 5.16% hydrogen, and 48.68% fluorine? The molar mass of the compound is 156.12 g/mol

Answer 1

Ans: Molecular formula = C₆H₈F₄

Given:

% C = 46.16

%H = 5.16

%F = 48.68

Calculate the # moles of each element:

moles of C = 46.16/12 = 3.847

moles of H = 5.16/1 = 5.16

moles of F = 48.68/19 = 2.562

Calculate the mole ratio:

C = 3.847/2.562 = 1.50

H = 5.16/2.562 = 2.0

F = 2.562/2,562 = 1.0

Empirical formula = C(1.5)H(2)F

Empirical formula mass = 12*1.5 + 1* 2+ 1*19 = 39 g/mol

Molecular mass = 156.12 g/mol

Ratio (n) = 156.12/39 = 4

Molecular formula = n(empirical formula) = 4(C1.5H2F) = C6H8F4

Answer 2

The molecular formula for a compound that is 46.16% carbon, 5.16% hydrogen, and 48.68% fluorine is C6H8F4.

HOW TO CALCULATE MOLECULAR FORMULA?

The molecular formula of a compound can be derived from the empirical formula, which can be calculated as follows:

• % C = 46.16
• % H = 5.16
• % F = 48.68

Next, we calculate the no. of moles of each element:

• moles of C = 46.16/12 = 3.847
• moles of H = 5.16/1 = 5.16
• moles of F = 48.68/19 = 2.562

Next, we calculate the mole ratio:

• C = 3.847/2.562 = 1.50
• H = 5.16/2.562 = 2.0
• F = 2.562/2.562 = 1.0

Empirical formula = C3H4F2

Empirical formula mass = (12 × 3) + (1 × 4) + (2 × 19) = 78g/mol

Molecular mass = 156.12 g/mol

Ratio (n) = 156.12/78 = 2

Molecular formula = n(empirical formula) = 2(C3H4F2) = C6H8F4

Therefore, the molecular formula of a compound that is 46.16% carbon, 5.16% hydrogen, and 48.68% fluorine is C6H8F4.

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