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Answered 2016-03-16 14:23:58

The empirical formula tells you the simplest formula for the compound. The molecular formula will be some multiple of the empirical formula, or it can be identical to the empirical formula.

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Answered 2016-03-16 20:43:21

These formulas indicates the chemical composition of a compound.

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CH4 has the same molecular and empirical formulas.




Empirical formulas are the result of chemical analysis of a compound.


Molecular formula is the integral multiple of Empirical formula.


Molecular formulas are used the most often, but empirical formulas do help at times. Often it's just to simplify the molecular formula, but this simplification can often tell you if it's in the same chemical family as other compounds and such.


Example of Empirical formula is : CO2 Example of Molecular formula is : C4O8


The similarity Is that you can find the components of the compound from both formulas



An empirical formula is a brutto formula; a molecular formula explain the structure of a molecule.


C2N2H8 can be reduced to an empirical formula by dividing all the numbers by 2. So its empirical formula is CNH4. None of the others can be reduced so they are all empirical formulas.


The empirical formula for nitrogen dioxide is the same as its molecular formula - NO2. See related question below for more details on how to find empirical formulas.


"Molecular formulas show the total number of each atom in the molecule. Empirical formulas only show the ratio of the elements in the molecule. For example - acetate Molecular Formula Empirical Formula C6H12O6 CH2O " I just wanted to note that although this is correct the chemical formula in the example "C6H12O6" is not acetate. It is glucose. Acetate is a derivative of acetic acid.


The same as its molecular formula; CH4. See related question below for more details on how to find empirical formulas.


Ca3P2 or Ca3(PO4)2 See related question below for more details on how to find empirical formulas.


Yes they can. For example CH2O is the empirical formula for both formaldehyde(CH2O) and glucose(C6H12O6)


An empirical formula is elaborated after the chemical analysis of a compound; for a structural formula more in depth studies are necessary.


An empirical formula represents the lowest whole-number ratio of ions or atoms in a compound. The formulas for ionic compounds are always empirical, because the proportions of the ions are always reduced to the lowest whole-number ratio. The formulas for covalent compounds are sometimes empirical, in which case they are also the molecular formulas. For example, the formula for water, H2O, is an empirical/molecular formula because the ratio of hydrogen to oxygen atoms is 2:1, which represents the lowest whole-number ratio of atoms in a molecule of water.


Empirical formulas determine the ratio of atoms of different elements within a chemical compound and can be derived by dividing the number of each element's atoms by their greatest common factor. They do not necessarily describe the full chemical makeup of a molecule. For example, benzene has the formula C6H6 but its empirical formula is simply CH because there is one hydrogen atom for every carbon atom. Glucose has the molecular formula of C6H12O6; its empirical formula is CH2O. Because the molecular formula for water, H2O, cannot be further simplified (empirical formulas have only whole numbers) H20 is also its empirical formula.


The emprical formula is C5H4. The molecular formula is C10H8.



The empirical formula of a compound does not tell you how the atoms are connected within the molecule. Most legislatures share the same empirical process for introducing bills.


Empirical formulas are used in ionic compounds because of simplicity. They are easier to describe with this type of formula because of their many crystals.


For sodium oxide, the empirical formula is the same as the formula unit, Na2O. (If any formula unit or molecular formula contains an atomic symbol with no following subscript, the empirical and actual formulas will be the same.)


The molecular formula is the same as the empirical formula, NO2. The compound NO2 has a molar mass of 46g/mol, so the empirical and molecular formulas are the same.



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