MOLE
CONCEPT



OBJECTIVES
Use the mole concept to express mass
of substances
Perform some calculations involving
mole, mass, percentage composition,
and empirical and molecular formulas
Infer the significance of the mole
concept.
What’s the word?
SAMS
MASS
OLME
MOLE
TOMICA
AMSS
ATOMIC
MASS
REPENTCAGE
PERCENTAGE
MOPCOSINIOT
COMPOSITION
1 pair = 2
1 DOZEN = 12
1 ream = 500
23
1 MOLE = 6.02 X 10
AVOGADRO’S NUMBER
602,200,000,000,000,000,000,000
TRIVIA TIME!
AMADEO AVOGADRO
AVOGADRO’S NUMBER
●
It is the number of particles
found in one mole of a
substance. It is the number of
atoms in exactly 12 grams of
Carbon-12
WHAT is
MOLE?
MOLE (Abbreviated mol)
MOLE
1.
2.
3.
It is fundamental (SI) unit used to measure the
amount of substance. In Latin, mole means a
‘massive heap” of material.
It can be defined as the number equal to the
number of Carbon atoms in 12.01 grams of
Carbon.
A mole is also the atomic or formula mass of a
substance expressed in grams.
DON’T FORGET!
Unlocking of Terms:


Mole:
Molecules:
MOLE TO MOLECULES
Example #1
How many Molecules are there in 4.0 moles of CO2?
Given: 4.0 mol of CO2
Find: Number of molecules of CO2
MOLES
MOLECULES
EXAMPLE #1
How many molecules are there in 4.0 moles of CO2?
EXAMPLE #2
Methane (CH4) is the simplest form of hydrocarbon. How
many moles are there in 3.01x1023 molecules of CH4?
MOLECULES TO MOLES
EXAMPLE #1
Water is said to be an excellent solvent. It can easily
dissolve polar and ionic solutes. How many water molecules
are there in 120 moles of water?
EXAMPLE #2
Sodium bicarbonate (NaHCO3) or baking soda is used in
baking. How many molecules are there in 100 moles of
sodium bicarbonate?
How much is in a
MOLE?
Calculating Moles and
Number of Atoms
Example #1
Aluminum (Al), a metal with high strength-to-weight
ratio and a high resistance to corrosion, is often used for
structures such as high-quality bicycle frames.
In a 10.0 gram of aluminum, compute the following:
a. Number of moles
b. Number of atoms
1 mol of Al = 26.98 g Al
ATOMS
MOLES
LET’S RECALL
Percent
Composition of
Compounds
OBJECTIVE

Determine the percent composition
of a compound given its chemical
formula and vice versa
Where do you see
PERCENTAGE?
Percent Composition
The percentage composition of an element in a
compound is equal to the ratio between the total mass
of an element in the compound and the molar mass of
an element in the compound multiplied by 100.
Percent Composition
10 grams of Coffee
13 grams of sugar
12 grams of milk
---------------------35 grams of 3 in 1 coffee
Calculate the percent composition of
coffee, sugar and milk in 3 in 1 coffee
sachet?
3 in 1 coffee
FORMULA
Example #1
Ethanol (C2H6O)
Ethanol (C2H6O)
Take Note!
1 mol of C2H6O molecules consists of 2 mol of carbon
atoms, 6 mol of hydrogen atoms and 1 mol of oxygen
atom.
CALCULATE THE PERCENT COMPOSITIONS OF
ETHANOL (C2H6O)
MOLAR MASS
CALCULATE THE PERCENT COMPOSITIONS OF
ETHANOL (C2H6O)
MASS PERCENT OF C
CALCULATE THE PERCENT COMPOSITIONS OF
ETHANOL (C2H6O)
MASS PERCENT OF H
CALCULATE THE PERCENT COMPOSITIONS OF
ETHANOL (C2H6O)
MASS PERCENT OF O
CALCULATE THE PERCENT COMPOSITIONS OF
ETHANOL (C2H6O)
MOLAR MASS
CALCULATE THE PERCENT COMPOSITIONS OF
ETHANOL (C2H6O)
Example #2
Glucose (C6H12O6)
What is the percentage composition of Carbon in
Glucose? Knowing that the molar mass of glucose is 180
g/mole and the total mass of carbon is 72 g/mole, the
percent composition is
Example #2
Glucose (C6H12O6)
Percent composition of Carbon =
LET’S RECALL
EMPIRICAL
FORMULA
EMPIRICAL FORMULA
The empirical formula (EF) is considered to be the
simplest formula of a compound. It is the smallest
possible whole-number ratio of the compound.
to determine the empirical
formula, follow these steps:
1.
2.
Using the atomic masses of each element, compute the
number of moles of each element.
From the computed number of moles, use the lowest
number as divisor for each element.
Example #1:
Compute for the empirical formula of the following:
42.11 g Carbon, 6.43 g Hydrogen and 51.46 g of Oxygen. Using the
atomic masses of each element, compute the number of moles
of each element.
Example #1:
From the computed number of molecules, use the lowest
number as divisor for each element. In this example, the divisor
will be 3.22 mol.
Example #2:
Compute for the empirical formula of the following:
32.65 g Sulfur, 65.3 g Oxygen and 2.04 g of Hydrogen. Using the
atomic masses of each element, compute the number of moles
of each element.
Example #2:
From the computed number of molecules, use the lowest
number as divisor for each element. In this example, the divisor
will be 1.02 mol.
Percentage
Composition
(PERFOMANCE TASK)
OBJECTIVES:
● Apply the concept of percentage composition in choosing grocery
items and
● Realize that the amount of substance intake can be monitored with
the use of percentage composition.
MATERIALS:
Grocery item containers or packages (food wrappers, can, bottles,
scissors), calculator, paper and pen.
PROCEDURE:
1. Get 3 samples of containers or packages of grocery items
such as canned goods, snacks, and beverages.
2. List the substances written as contents/ingredients on the
label.
3. Get the amount of Sodium per serving.
4. Compute for the percentage composition of the sodium of the
product based on the RENI’s Recommended Sodium intake =
2,400mg
290mg
X 100 = 12.08 % of Na
PERCENTAGE COMPOSITION OF SODIUM (Na) =
2,400mg
(RENI)
END