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Course: Stoichiometric Relationship
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Empirical Formulae and Molecular Formulae

Initially, chemical formulas were obtained by determination of masses of all the elements that are combined to form a molecule and subsequently we come up with two important types of formulas in chemistry : molecular formula and empirical formula.

The empirical formula of a compound gives the simplest ratio of the number of different atoms present, whereas the molecular formula gives the actual number of each different atom present in a molecule. If the formula is simplified then it is an empirical formula. The molecular formula is commonly used and is a multiple of the empirical formula.

The general statement relating molecular formula and the empirical formula is

Molecular Formula = n x Empirical Formula

 

What is Molecular formula?

        The molecular formula is the formula derived from molecules and is representative of the total number of individual atoms present in a molecule of a compound.

        A molecular formula uses a subscript that reports the actual number of each type of atom in a molecule of the compound.

        Molecular formulas are associated with gram molecular masses that are simple whole number multiples of the corresponding empirical formula mass.

 

What is Empirical formula?

        The empirical formula is the simplest formula for a compound which is defined as the ratio of subscripts of the smallest possible whole number of the elements present in the formula. It is also known as the simplest formula.

 

 

 

 

        An empirical formula for a compound is the formula of a substance written with the smallest integer subscript.

        The empirical formula gives information about the ratio of numbers of atoms in the compound. The percent composition of a compound directly leads to its empirical formula. Empirical Formula Vs Molecular Formula.

 

 

Empirical Formula

Molecular Formula

An empirical formula represents the simplest whole-number ratio of various atoms present in a compound 

The molecular formula shows the exact number of different types of atoms present in a molecule of a compound. 

Example : The empirical formula for Acetylene is CH .

Example : The molecular formula for Acetylene is C2H2 .

 

Example : Glucose Molecular Formula Vs Glucose Empirical Formula

Let’s take the example of glucose. The molecular formula of glucose is C6H12O6 and the empirical formula of glucose is CH2O. We can derive a relation between the Molecular formula and the empirical formula of glucose.

 

Empirical Formula & Molecular Formula of Butane & Octane [/caption]

C6H12O6 = 6 × CH2O

We can derive a general expression as,

Molecular formula = n x empirical formula where n is a whole number

Sometimes, the empirical formula and molecular formula both can be the same.

 

 

 

 

 

 

Question-1 : The empirical formula of Boron Hydride is BH3. Calculate the molecular formula when the measured mass of the compound is 27.66.

 

Solution : 

The atomic mass is given by = B + 3(H) = 10.81 + 3(1) = 13.81 u

But, the measured molecular mass for Boron atom is given as 27.66 u.  By using the expression,

Molecular formula = n x empirical formula n

                             = molecular formula/empirical formula

                             = 27.66 / 13.81

                             = 2

 

Putting the value of n = 2 in the empirical formula we get molecular formula as Molecular formula = 2(BH3) = B2H6.

 

 

 

Question-2 : The empirical formula of a compound is COCI2 and its molecular mass is 90.00u. Find out the molecular formula of that compound.

 

Solution :

COCI2 = C + O + 2(CI) = 12 + 16 + 2(35.5) = 99u

Empirical formula is the same as molecular mass as n=1, this means molecular formula is COCI2.

 

 

 

Question-3 : What is the molecular formula of a compound which has an empirical formula of CH2 and a relative molecular mass of 70?

 

Solution :

Relative molecular mass = 70

Empirical formula mass = 12 + 2 = 14

 

The relative molecular mass is 5 x the relative empirical formula mass

The molecular formula is 5 x the empirical formula The molecular formula is C5H10 .

 

 

 

Question-4 : A compound of iron and oxygen is analysed and found to contain 69.94% iron and 30.06% oxygen. Find the empirical formula of the compound.

 

 

Solution :

 

Steps       for Problem

Solving  

Find the empirical formula of a compound of 69.94% iron and 30.06% oxygen.

Identify    the        “Given information and what the problem is asking you to find.”

Given : 

% of Fe = 69.94%

% of O = 30.06%

Find : Empirical Formula = Fe?O?

                                                Calculate

a. Assume a 100g sample, convert the same % value to grams.  

69.94g Fe

30.06g O

b. Covert to moles.

69.94g Fe x 1 mol Fe   = 1.252 mol Fe 

                    55.85g Fe

 

30.06g O x  1 mol O   = 1.879 mol O 

                   16.00g O 

c. Divide both moles by the smallest of the results.

          Fe x  1 .252 mol  

                       1.252

 

           O x  1.879 mol  

                      1.252

The “non-whole” empirical formula of the compound is Fe1O1.5

 

d. Multiply each of the moles by the smallest whole number that will convert each into a whole number.

Since the moles of O is still not a whole number, both moles can be multiplied by 2, while rounding to a whole number.

e. Write the empirical formula 

The empirical of the compound is Fe2O3

                

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