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2010-11-09 07:20:32
2010-11-09 07:20:32

There are 4 step to determine molecular formula, which are given bellow

Step:1:- Find empirical formula

Step:2:- Find empirical formula mass

Step:3:- Find n

n=molecular mass/empirical formula mass

Step:4:- now find molecular formula to find molecular formula

molecular formula(empirical formula)n


Related Questions

By determining the molecular mass, then dividing the molecular mass by the formula mass of the empirical formula to determine by what integer the subscripts in the empirical formula must be multiplied to produce the molecular formula with the experimentally determined molecular mass.

the empirical formula and the molar mass

A molecular formula comprises the constituent atoms of a molecule; to determine molecular mass, summate the atomic masses of the elements in their respective proportions.

Not completely. The empirical formula of a substance can be determined from its percent composition, but a determination of molecular weight is needed to decide which multiple of the empirical formula represents the molecular formula.

Calculate the empirical formula weight. Find the ratio of the molecular weight to the empirical formula weight. (n= molecular weight/ empirical formular weight). Multiply each subscript of the empirical formula by n.

From the percentage composition only, an empirical formula can be derived, but a proper molecular formula can only be assured by adding some information about the molecular weight of the substance concerned.

In order to find molecular formula from empirical formula, one needs to know the molar mass of the molecular formula. Then you simply divide the molar mass of the molecular formula by the molar mass of the empirical formula to find out how many empirical formulae are in the molecular formula. Then you multiply the subscripts in the empirical formula by that number.

The actual mass must be divided by the empirical mass. This was derived from the following equation: (subscript)(empirical formula) = (molecular formula) subscript = (molecular formula)/(empirical formula)

A molecular formula is the same as or a multiple of the empirical formula. The first step will be to assume exactly 100 grams of the substance, then convert each of these masses to moles,

The empirical formula is the formula in its most simplified terms. The molecular formula is how many moles there actually are (the empirical formulat multiplied by a factor).

Because unlike the empirical formula, the molecular formula does not have to be the simplest ratio.If by chance you are given the percent composition of the elements in a substance, you could calculate the empirical formula and then the empirical formula's mass. However, the molecular formula equation is molecular formula= (empirical formula)n, where n is the mass of the molecular formula divided by the mass of the empirical formula. You would, therefore, need to know the mass belonging to the molecular formula, which you are not given.

molar mass of unknown/molar mass of empirial = # of empirical units in the molecular formula. Example: empirical formula is CH2O with a molar mass of 30. If the molar mass of the unknown is 180, then 180/30 = 6 and molecular formula will be C6H12O6

Add up or Tally the number of atoms of C, and H, and O and there you have it; namely Glucose = C6, O6, H12 is its molecular formula..

The microwave does not have a molecular formula. It is the foods that we heat in a microwave that has the molecular formula.

Molecular formula is the actual representation of the constitution of the substancewhile Empirical formula is the simplest representation of the molecular formula.Molecular formula= Empirical formula*n(where n= Molecular weight/Empirical formula weight)Example :-EtheneMolecular formula =C2H4Empirical formula=CH2here CH2 is the simplest representation of molecular formula of Ethene.

Because an empirical formula is the simplest form of a compound, we know that the molecular formula contains more atoms than it does. Since we are given the molar mass, we can use this formula. x ( MM of empirical formula ) = MM of molecular formula MM of empirical formula = 12(2) + 1(6) + 16 = 46 MM of molecular formula = 138 46x = 138 x= 138 / 46 x=3 Therefore, the molecular formula is 3(C2H6O) that is C6H18O3 must know the molecular weight 2.compute the ratio of molecular weight to formula weight 3.multiply all subscripts in the empirical formula by this ratio

The molecular formula for Ethanol is CH3CH2OH The molecular formula for Ethylene is C2H4

the molecular formula for cholesterol is C27H46O

C4H4O is the molecular formula

the molecular name of urea is diminomethanal and molecular formula is ch4n2o

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