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Answer: The empirical formula for the given compound is and molecular formula for the given compound is
Explanation : Given,
Mass of C = 18.24 g
Mass of H = 0.51 g
Mass of F = 16.91 g
To formulate the empirical formula, we need to follow some steps:
Step 1: Converting the given masses into moles.
Moles of Carbon =
Moles of Hydrogen =
Moles of Fluorine =
Step 2: Calculating the mole ratio of the given elements.
For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.51 moles.
For Carbon =
For Hydrogen =
For Fluorine =
Step 3: Taking the mole ratio as their subscripts.
The ratio of C : H : F = 3 : 1 : 2
The empirical formula for the given compound is
For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.
The equation used to calculate the valency is :
We are given:
Molar mass = 562.0 g/mol
Mass of empirical formula = 3(12) + 1(1) + 2(19) = 75 g/eq
Putting values in above equation, we get:
Multiplying this valency by the subscript of every element of empirical formula, we get:
Thus, the molecular formula for the given compound is