Empirical Formula and Molecular Formula
Empirical Formula shows the simplest whole-number ratio of the elements in a compound. Molecular Formula indicates the exact number of each type of atom in a molecule. It may be the same as the empirical formula or a multiple of it.
1.0Molecular Formula
- Represents the actual number of each type of atom present in a molecule.
- Uses subscripts to indicate the exact count of each atom in a molecule.
- Reflects the true composition of a compound, not simplified.
- The molecular mass (or molar mass) of a compound corresponds to a whole-number multiple of the empirical formula mass.
- Example: The molecular formula for glucose is C6H12O6, showing that each molecule contains 6 carbon, 12 hydrogen, and 6 oxygen atoms.
2.0Empirical Formula
The empirical formula of a compound represents the simplest whole-number ratio of atoms of each element present in the compound. It gives the relative number of atoms rather than the actual number in a molecule.
- Represents the simplest whole-number ratio of the elements in a compound.
- Provides a reduced or simplified version of the formula, focusing on the ratio, not the exact count.
- Known as the "simplest formula" because it only shows the basic proportional relationship between elements.
- The empirical formula is derived directly from the per cent composition of the compound.
- Example: The empirical formula for glucose is CH2O, indicating the simplest ratio of carbon, hydrogen, and oxygen is 1:2:1.
3.0Steps to Calculate the Empirical Formula
- Determine the Mass of Each Element: Use the given data or assume a 100 g sample if percentages are provided.
- Convert Mass to Moles: Use the formula: Moles of an element=Mass of the element (g)Atomic mass of the element (g/mol)Moles of an element=Atomic mass of the element (g/mol)Mass of the element (g)
- Find the Simplest Whole-Number Ratio: Divide all mole values by the smallest number of moles calculated.
- Write the Empirical Formula: Use the ratio of moles as subscripts in the formula. If the ratios are not whole numbers, multiply by the smallest integer that converts them to whole number
Example
Glucose:
- Percent composition: C: 40%, H: 6.7%, O: 53.3%
- Empirical formula: CH2O
Hydrogen Peroxide:
- Simplest ratio: HO
Solved Example
- Calculation of the Empirical Formula of Phosphoric Acid
Given Composition:
- Hydrogen (H): 3.06%
- Phosphorus (P): 31.63%
- Oxygen (O): 65.31%
Solution:
Assume 100 g of the compound:
- This simplifies the percentages directly into masses:
- Mass of H = 3.06 g
- Mass of P = 31.63
- Mass of O = 65.31 g
Calculate the number of moles for each element:
- Using the formula:
- For H, Moles of H = (3.06)/1 =3.06
- For P. Moles of P = (31.63)/31 = 1.02
- For O, Moles of O = (65.31)/16 =4.08
Find the simplest ratio of moles:
- Divide all the mole values by the smallest number of moles, 1.02
- Ratio of H =
- Ratio of P =
- Ratio of O =
Write the empirical formula:
- Use these ratios as subscripts for the elements:
- Empirical formula = H3PO4
Solved Example
- Glucose:
Empirical formula: CH2O
Empirical formula mass: 12+2(1)+16=30 g/mol
Molar mass: 180 g
n = 180/30 = 6
Molecular formula: C6H12O6
- Hydrogen Peroxide:
Empirical formula: HO
Empirical formula mass: 1+16=17 g/mol
Molar mass: 34 g/mol
n = 34/17 = 2
Molecular formula: H2O2
4.0Process to Determine the Molecular Formula from the Empirical Formula
Determine the Empirical Formula:
- Start with the per cent composition or the masses of each element in the compound.
- Convert these masses to moles.
- Find the simplest whole-number ratio of the elements, which gives you the empirical formula.
Calculate the Empirical Formula Mass:
- Add up the atomic masses of all the elements in the empirical formula. This gives you the empirical formula mass.
Determine the Molecular Weight (Molar Mass) of the Compound:
- The molar mass (usually given in the problem) is the actual mass of one mole of the compound.
- This value is needed to relate the empirical formula to the molecular formula.
Find the Integer Multiple (n):
- Use the formula:
- This integer n tells you how many times the empirical formula must be multiplied to obtain the molecular formula.
Calculate the Molecular Formula:
- Multiply each subscript in the empirical formula by the integer n.
- The result gives the molecular formula.
Solved Example
Empirical formula: CH2
The molar mass of the compound: is 84 g/mol
Steps:
- Empirical Formula Mass:
Carbon (C): 12 g/mol
Hydrogen (H): 2×1 g/mol = 2 g/mol
Empirical formula mass = 12+2 = 14 g/mol
- Find the Integer Multiple n:
n = 8414 = 6
- Determine the Molecular Formula:
Multiply each subscript in CH2 by 6.
Molecular formula: C6H12.
5.0Differences Between Empirical and Molecular Formulas
Frequently Asked Questions
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