The molar mass of a chemical compound in chemistry is defined as the mass of a sample divided by the amount of substance in the sample that is measured in moles.
The molecular weight is usually used as a synonym of molar mass especially for molecular compounds, although it is very different as is known as molecular mass.
Molar mass is a smallest unit of a compound with one twelfth of the mass of one carbon – 12 atoms. When we know the number of moles needed, the concept of molar mass can be used to calculate how many grams of substance are required. The molar mass otherwise known as molecular weight is the sum of the total mass in grams of all the atoms that make up a mole of a molecule. The unit required to measure is grams per mole.
Mass of 1 mole of atom = Ar in grams
Number of moles of atom = mass of the element in grams/ relative atomic mass, Ar
Mass of 1 mole of molecules = Mr in grams
Number of moles of molecules = mass of the substance in grams / relative molecular mass, Mr
Mass of substance the contains 1 mole of particle = molar mass
Percentage yield = actual mass of product obtained / theoretical mass of product obtainable.
A mole is the SI measure of the quantity of a ‘chemical entity’ such as electrons, protons, or atoms. 1 mole contains 6.022 × 1023 elementary entities of the substance. Avogadro’s number is fundamental for understanding both the makeup of molecules and their combinations and interactions. For instance, since one atom of oxygen combines two atoms of hydrogen to create one molecule of water (H2O), one mole of oxygen (6.022 × 1023 of O atoms) combines with two moles of hydrogen (2 × 6.022 × 1023 of H atoms) to make one mole of H2O.
Another Avogadro’s number property is that the mass of one mole of a substance is equal to the molecular weight of the substance. For instance, the mean molecular weight of water is 18.015 atomic mass units. Therefore, one mole of water weighs 18.015 grams. It simplifies many chemical computation.
Compounds are those substances that are made up of one or more elements. Examples of some common compounds include glucose, salt, acetic acid, and sodium bicarbonate.
Sodium chloride compound is made up of two elements i.e., sodium and chloride. We will use sodium chloride as one of the examples to calculate the molar mass for the compounds
Step 1: Find the atomic mass of individual element in the periodic table
We have to first find the atomic mass for each element. The element sodium has the atomic mass of 22.98976g/mol. Chlorine has an atomic mass of 35.453 g/mol.
Step 2: Count atoms for each element
As there are no subscripts for compound sodium chloride, it means it has only one sodium and one chlorine atom for the compound.
Step 3: find the molar mass
Now, we are able to find the molar mass as we know the number of atoms for each element. Here we calculate first the mass of the sodium atoms that is 22.98976 g/mol. we will repeat the same for mass of chlorine atoms that is 35.453 g/mol, now we have to add these two masses together to find the total mass of molecules of sodium chloride. The total sodium chloride molecules are 58.44276 g/mol which we can round up to 58.44 g/mol.
Na = 1 × (22.98976 g/mol) = 22.98976 g/mol
Cl = 1 × (35.453 g/mol) = 35.453 g/mol
Molar mass = 22.98976 + 35.453 g/mol
Molar mass = 58.44276 or 58.44 g/mol
1. When you have 1.25 grams of a molecule with a molecular weight of 134.1 g/mol, find out how many moles of that molecule you have?
Solution: 1.25 g × 1 mole / 134.1 g = 0.0093 grams.
2. Calculate the mass of 6.022 × 1023 molecules of NH4Cl?
Solution: Molar mass in grams of NH4Cl = 14 + 4 +35.5 = 53.5 g
No. of moles of NH4Cl = 6.022 × 1023 / 6.022 × 1023 = 1 mole.
Now, mass of NH4Cl = number of moles × molar mass
= 1 × 53.5 g
= 53.5 g
3. Calculate the number of methane molecules and the number of carbon and hydrogen atoms in 25 g of methane?
Solution: Molar mass of methane = 16
Number of methane molecules = 25/16 × 6.022 × 1023
= 9.411 × 1023
Number of carbon molecules = 1 × 9.411 × 1023
= 9.411 × 1023
Number of hydrogen molecules = 4 × 9.411 × 1023
= 3.74 × 1023
1. What is the Need and Use of Mole Concept?
Mole concept allows chemistry to weigh quantities of two substances, for instance, sulphur and iron, to get an equal number of atoms of sulphur and iron. As it is a chemical quantity unit, it connects the atom with the macroscopic quantities of material by which we work in the laboratory. A substance mole is a material mass containing the same number of basic units as atoms in exactly 12000 g of 12C.
2. Why is Avogadro’s Number Called a Mole and What Does its Law State?
The atomic mass unit of an element is the density of one mole in grams in weight. A few years later the French physicist Jean Perrin called the number of units in the sum of one mole Avogadro. The law of Avogadro also considered as rule or theory of Avogadro is an experimental gas law that relates the value of gas to the amount of gas present. The law states that equal quantities of all gases have the same number of molecules at same pressure and temperature.