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Every matter has its own properties. Matter has
three states that differ from each other. Their
differences in their properties are based on the
arrangement of their particles. Under normal
atmospheric condition, there are only 11
elements that are gases (diatomic molecules
hydrogen, nitrogen, oxygen, fluorine, and
chlorine and the noble gases helium, neon,
argon, krypton, xenon, and radon. Ozone,
another form of oxygen, is also a gas at room
temperature.

Volume
• Molecules of gases
occupy a space. It
may be proven
when the gas fills
up its container
.
• 1 L = 10 dm = 10
m = 1000 mL =
1000 cm
• Its SI is in liters (L).
It can also be
expressed in
milliliters (mL),
cubic centimeters,
Pressure Temperature Amount of gas
3 3
3
3
• The physical force
exerted on an
object. Pressure of
the gas is the force
exerted by the gas
per unit area.
• Pressure(P) = Force
(F) / Area (A)
• 1 atm = 760 mm of
Hg = 760 torr =
1.01325 bar =
101.325 kPa
• The SI unit used for
• The temperature
of a gas depends
on the kinetic
energy of the gas.
Gases expand
when temperature
is increased.
• K= C + 273.15
• The temperature
of the gas is
generally
expressed in
Fahrenheit,
• The mass of the
gas is related to
the number of
moles of the gas.
• number of moles
(n) = mass of the
gas / molar mass
of the gas
• The mass of the
gas is generally
expressed in
kilograms (kg) or
grams (g)
Fundamental Properties
of Gas

• The behavior of gases is determined by
the behavior of its individual particles.
• The kinetic molecular theory was
formulated using a simple model.
• In 1870, scientist were able to make a
model of ideal gas or theoretical gas.
• The particles of an ideal gas behave
consistently and in a predictable manner.
• It serves as a basis which attempts to
explain the behavior of real gases.
Kinetic
Molecular
Theory

Characteristics of
Gas
Gases like any
other states of
matter, consists
of very tiny
particles, each of
which has mass.
The density of
gases varies with
changes in
temperature and
pressure.
Gases are most likely
empty space because
of a wide distance
between these tiny
particles. Thus,
making gases
compressible and
have low density.

Characteristics of
Gas
Gas particles
move rapidly in
straight lines,
travel constantly
and in random
directions.
Because of the
wide spaces
between gas
particles, the
forces of attraction
(Van der Waals
Force) between
them are
negligible.
Gases diffuse very
rapidly that allows
two or more gases
to mix readily
when combined.

Characteristics of
Gas
Gas particles collide with
each other or with the
walls of its container but
do not lose their kinetic
energy; instead, it is only
transferred to the lower-
energy particle and will
continue to move. In short,
energy is conserved in
All gases have the same
average kinetic energy at a
given temperature of gas.
The average kinetic energy
of gas particles is directly
proportional to the absolute
temperature of the gas. this
means that gas particles
may have higher kinetic
energy at a higher

The four measurable properties of gases such
as pressure, volume, temperature, and number
of moles are related to each other.
There are four main gas laws. These are Boyle’s
Law, Charles’ Law, Gay-Lussac’s Law, and
Avogadro’s Law. These laws are products of
various experiments that are done many
centuries ago. The Ideal Gas Law can be used
to describe the relationship between variables
used by the four main gas laws.

• Proposed by Robert Boyle, an Anglo-Irish
chemist.
• He investigate the relationship between
pressure and volume of a gas using a J-
shaped tube apparatus.
• He proposed that the volume of a given
mass of gas held at constant temperature
is inversely proportional to its pressure.
• Boyle shown that as the volume decreases,
the pressure increases.
BOYLE’S
LAW

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Describing Gases_20250304_144557_0000.pptx

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