Relative Atomic Mass of Elements
Before we get to talking about moles, we need to cover relative masses.
The relative atomic mass of an element is the ratio of the average mass of one atom of a specific element compared to 1/12 the mass of one atom of carbon-12. Relative atomic mass is dimensionless, that is, it has no units.
Carbon-12 is assigned a mass of exactly 12.00 atomic mass units.
For example, to find the relative atomic mass of hydrogen, we divide the mass of 1 hydrogen atom by 1/12 the mass of 1 atom of carbon:
(1.67 × 10^-27 kg)/ (1/12)(2.00 × 10^-26) = 1
The relative atomic mass of hydrogen is 1.
Relative Molecular Mass of Compounds
The relative molecular mass is the average mass of one molecule or formula unit of the compound compared with 1/12 the mass of one atom of carbon-12.
Finding the relative molecular mass is fairly simple:
Write the chemical formula of the compound
Identify the atoms or ions present
Multiply the relative atomic mass of each atom or ion by the number of like atoms present in the compound
Add all the numbers.
The term mole is similar to the word "dozen," or "pair," because it represents a specific, fixed number of objects. In the same way that dozen refers to 12 items, or pair refers to 2, mole constitutes a fixed number of particles.
The mole is the amount of substance which contains as many particles (whether ions, atoms or molecules) as there are atoms in 12 grams of carbon-12.
(You will find that lots of measurements in Chemistry are based around the Carbon-12 isotope).
To show you the number of atoms present in 12 grams of carbon-12, which is the number or particles in a mole, we can perform a calculation:
The mass of one carbon-12 atom is: 1.99 × 10^-26 kg, or 1.99 × 10^-23 g
Therefore, the number of carbon atoms in 12 grams of carbon-12 will be:
12 g/1.99 × 10^-23 g = 6.023 × 10^23
This number, when rounded off, is approximately 6.0 × 10^23, known as Avogadro's Number, the number of particles in one mole of a substance.
This is the chemical equivalent as knowing that a dozen is twelve- one mole corresponds to the same number of particles in every chemical substance.
Now that you know how many particles are in a mole of any substance (Avogadro's Number), you can find the molar mass of a chemical substance.
The molar mass is the mass in grams of 1 mole of a specific substance, and you find it by multiplying the mass of one atom of the element by Avogadro's Number.
Using hydrogen as an example again:
Molar mass of hydrogen = (1.67 × 10^-24 g) × (6.0 × 10^23) = 1 g/mol
You will realize that the molar mass of hydrogen is the same value as the relative atomic mass, however, relative atomic mass has no units, while molar mass is measured in g/mol (or gmol^-1).
Note: There is a difference between one mole of atoms and one mole of molecules, especially in molecular elements like chlorine, nitrogen and hydrogen gas (which exist as diatomic molecules).
1 mole of atoms is 6 × 10^23 atoms.
1 mole of molecules is 6 × 10^23 molecules.
Conversions Involving the Mole
At this point, you know about moles, how they relate to Avogadro's number and the number of particles in a mole, and relative atomic masses. CSEC requires you to know how to perform certain calculations and conversions with the information given to you.
Converting Mass to Moles
number of moles= (given mass in grams of element or compound)/(molar mass of element or compound)
Simply divide the mass of the substance mentioned in the question by the molar mass of the substance.
For example: What is the number of moles of sodium chloride formula units present in 1.17g of sodium chloride?
The mass of 1 mole of NaCl = 23+35.5= 58.5 g/mol
Hence, 58.5 g of NaCl contains 1 mole of NaCl formula units.
1.17g NaCl will contain (1.17/58.5) = 0.02 mol of NaCl formula units
Converting Moles to Mass
mass of a certain number of moles= molar mass × number of moles
For example: What is the mass of 0.25 moles of nitric acid?
Molar mass of nitric acid= [1+14+(3×16)]= 63 g/mol
Hence, the mass of 0.25 moles of nitric acid= 0.25 × 63 g/mol= 15.75 g
Converting Moles to Number of Particles
number of particles= Avogadro's Number(L) × number of moles
Example: How many particles are in 3.5 moles of Lithium?
# of particles= 3.5 × 6.0×10^23 = 2.1 × 10^24
Converting Number of Particles to Moles
number of moles= number of particles/Avogadro's Number(L)
Example: How many moles of silicon would contain 3.72 × 10^24 particles?