Molecular Mass

# What is the molecular formula of a compound with an empirical formula of CH and a molecular mass of 78?

###### Wiki User

CH = 13 so 78/13 = 6 The compound is C6H6 = benzene (most likely).

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## Related Questions

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.

If you know the molar mass of the compound, you have to calculate the mass of the empirical formula and divide the molar mass of the compound by the mass of the empirical formula in order to find the ratio between the molecular formula and the empirical formula. Then multiply all the atoms by this ratio to find the molecular formula!

Yes, the empirical formula is the most basic ratio of the elements in a compound, while the molecular formula is the ratio in a compound. For instance C5H10O could be both the empirical and the molecular formula or the molecular formula could be C10H20O2 the molecular formula depends on the molar mass.

C4H6. C2H3 gives a molecular mass of 27, 54/27 gives 2. Therefore the molecular formula is twice the empirical formula.

The formula of NO2 has a molecular weight of 46 g/mol. Your compound has a molecular weight of 92 g/mol. As you can see the molecular weight of the compound is twice that of the empirical formula. Therefore the molecular formula of your compound is:2 *(NO2) ---> N2O4

The molecular formula of this compound is N2H2. This is obvious because the empirical formula of a compound is the lowest positive integer ratio of atoms present.

Since carbon has an atomic mass of 12 and hydrogen has an atomic mass of 1, the mass of the empirical formula is 12 + 3 = 15. 60/15 = 4; therefore, the molecular formula is C4H12.

the molecular mass of a compound and its empirical formula

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)

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 CH2 has a formula mass of 14, and 42.0/14 = 3. Therefore, the molecular formula is C3H6.

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.

If you mean to find its molecular formula: 1. First you must obtain the empirical formula. Find the molar mass of the empirical formula. 2. The molar mass of the entire molecule must be given or its molecular formula cannot be find. 3. Put the molar mass given over the molar mass of the empirical formula. 4. Use this number (kind of like a scaler) to multiply by the entire empirical formula. This is the molecular formula.

The empirical formula of SN has a formula unit mass of the sum of the gram atomic masses of nitrogen and sulfur, i.e., about 46.0667. The gram molecular mass given in the problem divided by this formula unit mass is about 4. Therefore, the molecular formula is S4N4.

The gram formula unit mass of the empirical formula C2H3 is twice the gram atomic mass of carbon plus three times the gram atomic mass of hydrogen, or about 27. The nearest integer to 162.27/27 is 6. Therefore, the molecular formula for the compound is C12H18.

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

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

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.

Mass?Here it is with an example.. a compound of 78.14% Boron and 21.86% hydrogen with an experimental mass of 27 to 28 g. The empirical formula is as above BH3and Molecular formula is B2H6Molar mass / by empirical formula mass should give you an integer to multiply the empirical formula (BH3) with. This time it was 2 (rounded).