Empirical and molecular formula

In summary, empirical and molecular formulas are two ways of representing the composition of a compound. The empirical formula shows the simplest whole number ratio of elements, while the molecular formula shows the actual number of each element in a molecule. To calculate the empirical formula, the mass of each element must be determined and converted to moles, and then divided by the smallest number of moles. The empirical formula is important because it allows for easy comparison of compounds. The molecular formula is either the same or a multiple of the empirical formula, with the multiple being determined by dividing the molecular mass by the empirical formula's molar mass. In some cases, a compound's empirical and molecular formula may be the same if the molecular formula is already the simplest whole number
  • #1
yaseen shah
32
0
please tell me a quick for determination of empirical and molecular formula and also who invented it.
 
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  • #2
There are no shortcuts. If you will use google you will find many tuorials on .edu sites.
 

What is the difference between empirical and molecular formula?

The empirical formula represents the simplest whole number ratio of elements present in a compound, while the molecular formula represents the actual number of each element present in a molecule.

How do you calculate the empirical formula?

To calculate the empirical formula, you need to determine the mass of each element present in the compound and convert it into moles. Then, divide each element's moles by the smallest number of moles to get the simplest whole number ratio.

What is the significance of the empirical formula in chemistry?

The empirical formula is important because it provides a simple way to represent the composition of a compound and allows for easy comparison of different compounds.

How is the molecular formula related to the empirical formula?

The molecular formula is either the same as or a multiple of the empirical formula. The multiple is determined by dividing the compound's molecular mass by the empirical formula's molar mass.

Can a compound have the same empirical and molecular formula?

Yes, in some cases, a compound's empirical and molecular formula may be the same. This occurs when the compound's molecular formula is already the simplest whole number ratio, so it cannot be reduced any further.

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