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Molar Mass Calculations and Molecular Weight Calculator

By Roberta Crowell Barbalace

In order to grasp the concept of molar mass calculations it is important to understand the molar unit. The mole also called mol is the basic unit of measurement in chemistry. By definition, in modern chemistry, one mole represents the number of carbon atoms in exactly 12 grams of carbon 12 isotope. Remember that carbon-12 has an atomic mass of 12 (six neutrons and six protons).

One mole of anything, however, contains 6.0221367E²³ of that object. This is known as Avogadro's number.

Examples:

1 mole of carbon = 6.0221367E²³ carbon atoms

1 mole of bananas = 6.0221367E²³ bananas
(Aren't you glad they don't sell bananas by the mole?)

Obviously it would be impossible to count out 6.0221367E²³ atoms. Remember, however that 1 mole of carbon-12 = 12 grams = 6.0221367E²³ atoms. It has been established that 1 mole of any element = the atomic mass of that element expressed in grams. Since magnesium has an atomic mass of 24, one mole of magnesium weighs 24 grams and contains 6.0221367E²³ atoms of magnesium. A mole of any molecule = the molecular mass of that molecule expressed in grams. In order to determine the weight of one mole of bananas, one would have to get an average weight of a banana and multiply that by 6.0221367E²³ then we could weigh out that weight of bananas and presto, we would have a mole of bananas. Of course, nobody would ever do that. It just demonstrates that mole of anything = 6.0221367E²³ and we can measure out a mole of something by counting it or by weighing it out. Since atoms are too small to count, we must weigh out a mole of atoms.

Molar massis a unit that enables scientists to calculate the weight of any chemical substance, be it an element or a compound. Molar mass is the sum of all of the atomic masses in a formula. Once one determines the molar mass of a substance, it will be easy to measure out one mole of that substance.

The molar mass calculation of a substance is complete the following steps (We will use sulfuric acid, H₂SO₄, as an example):

1. Make a list of each element and the number of atoms of each element present in the substance.

   H 2
   S 1
   O 4

2. Go to periodic table and determine the atomic mass average (atomic weight) of each element.

   H 1.00794
   S 32.066
   O 15.9994

3. Multiply each atomic mass by the number of atoms in the formula.

   H 1.00794 * 2 = 2.015
   S 32.066 * 1 = 32.066
   O 15.9994 * 4 = 63.998

4. Add up the results of step three:

   2.015+32.066+63.998 = 98.079 = molar mass of sulfuric acid

In this example the results have been rounded off to the correct number of decimal places. (Since the atomic mass average of sulfur given above only has 3 decimal places, accuracy can not be determined beyond that point).

These calculations will be necessary before one can determine the molarity or normality of a solution and many other formulas in stoichiometry (the quantitative relationships between chemical substances in a chemical equation).

Try these formulas and then compare your results to those you get on the calculator below:

H₂O

NH₃

C₂H₄O₂

K₂Cr₂O₇

Molecular Weight Calculator

Formulas can have a max of two brackets open at the same time, and the molecule of crystallization must be placed last.

Examples:

3BeO.Al2O₃.6(SiO₂) = (BeO)3.Al2O3.6(SiO2)

(BaH₂O)₂Mn₅O₁₀ = (BaH2O)2Mn5O10

(KMgCl₃).6H₂O = (KMgCl3).6H2O

Related Resources

• Molarity, Molality and Normality
  Introduces stoichiometry and explains the differences between molarity, molality and normality.
• Periodic Table of Elements
  Provides comprehensive data on the chemical elements including scores of properties, element names in many languages, chemical compounds, most known nuclides.
• Anatomy of the Atom
  Answers many questions regarding the structure of atoms.

Citing this page

If you need to cite this page, you can copy this text:

Roberta Barbalace, Kenneth Barbalace. Molar Mass Calculations and Molecular Weight Calculator. EnvironmentalChemistry.com. 1996. Accessed on-line: 11/22/2024
https://EnvironmentalChemistry.com/yogi/reference/molar.html
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