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

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

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explanation: