MOLE CONCEPT
Chemical reactions occur between large
number of particles, and these particles may be in the form of atoms, molecules
or ions and each of these particles has their own relative mass, but there is no
fit in between the amounts of each matter and its mass.
For example, if a student was asked
to compare 1 g of H2 gas and 1 g of N2 gas and 1 g of O2 gas
in terms of the number of particles it cannot solved for the simple reason that
the molecular masses of these elements vary from each other, the molecular mass
of hydrogen gas 2, nitrogen 28 and for oxygen 32. If the mass of 1 g is divide for
each item on the molecular mass.
Then values obtained can be used
for comparison. So, years ago, the need arose for independent units to express
the amount of substance and this unit had found general acceptance, this unit
is mole (mole) and symbolizes (n) and it is one of the basic units in the international
system of units, the mole defined as the quantity of material containing the same
number of particles (molecules, atoms or ions) containing in 12 g of carbon isotope
12 (12C) (where this isotope is used also as a measure to calculate atomic mass
as previously mentioned) and this number of particles called the Avogadro's Number)
which equals to 6.023 × 10*23 and symbolizes NA. It must be emphasized that Mole is the actual amount
of the matter and is not the mass.
The Mole is one of the most important
basic concepts in general chemistry and which adopted by scientists to
consolidate their theory to many important is- sues in chemistry. And we can apply
the concept of mole on atoms, molecules, ions or electrons so it is always necessary
to specify the type of particle that we deal with, for example,
· Mass of one mole of atoms of the isotope carbon-12 is
12 g
· Mass of one mole of atoms of silver is 107.868 g
· Mass of one mole of H2 molecules are 2 g
· Mass of one mole of ions SO4*2- is 96 g
And number of moles (n) is calculated
using the following relationship:
n (mol) = mass (m) (g) / molar mass (M) (g/mol)
Applications of Mole Concept
As we have told before, the mass of
1 mole of carbon atom is 12 grams. According to this, it is possible to
calculate the mass of 1 carbon atom.
We can write the following equation:
Number of moles =
Number of particles (atoms, ions or molecules)/ Avogadro's number
Example 1
a. Calculate the number of moles of
3.01×10*25 water molecules.
b. Calculate the number of molecules
in 0.02 mole of CO2.
Solution:
Example 2
Calculate the number of molecules
in 170 g of H2S gas.
Solution:
Exercises
1. What is the number of moles in 5.6 g of PCl5?
2. Calculate the number of molecules of SiO2 found in 1mg
of dust. (Assume that dust particles are made up of 100% SiO2.)
Comments
Post a Comment