This document discusses gas laws, including Boyle's law. It provides examples showing that for a fixed amount of gas at constant temperature, volume and pressure are inversely proportional. Specifically, it states that Boyle's law describes how doubling the pressure halves the volume of a gas, and halving the pressure doubles the volume, at constant temperature. It also provides sample problems and solutions demonstrating how to use Boyle's law equations to calculate changes in pressure or volume given one is fixed.

1. GAS LAWS
SIR JOHNEL V. ESPONILLA
G10 - SCIENCE

2. OBJECTIVES:
G A S
L AW S
1. Define atmospheric pressure
2. Explain why atmospheric pressure
decreases with increasing altitude
3. Describe how atmospheric pressure is
measured

3. THE EARTH’S ATMOSPHERE
G A S L A W S
The Earth’s atmosphere is principally a mixture of
elemental nitrogen and oxygen and other gases.

4. THE EARTH’S ATMOSPHERE
G A S L A W S
The Earth’s atmosphere is principally a mixture of
elemental nitrogen and oxygen and other gases.

5. COMPOSITION OF THE
EARTH’S ATMOSPHERE
G A S L A W S
Gases may exist as diatomic
molecules
An allotrope of oxygen is a gas at
room temperature
The noble gases are monatomic
gases
Gases may exist as diatomic
molecules
Other gases are molecular covalent
compounds

6. COMPOSITION OF THE
EARTH’S ATMOSPHERE
G A S L A W S
Most gases are colorless
Nitrogen is the major gas
The nitrogen can be converted
into nitrogen oxide during
lightning storms
Soil microbes are capable of
converting said nitrogen into
nitrates and ammonium salts
Oxygen is released into the
atmosphere as the result of the
photosynthetic reactions

7. ATMOSPHERIC PRESSURE
G A S L A W S
Pressure = Force over area
Atmospheric pressure is the
result of air molecules striking
various surfaces in the
environment.
How is it measured?

8. ATMOSPHERIC PRESSURE
G A S L A W S
How is it measured?
By barometer
Evangelista
Torricelli
invented the
barometer.
A barometer is a device used to
measure atmospheric pressure.

9. ATMOSPHERIC PRESSURE
G A S L A W S
The atmosphere is denser near the
surface of the Earth than in higher
altitude.
Forcearea = weightair column
The exact height of the mercury in the
tube depends on the atmospheric pressure
which varies with altitude.
At sea level: height = 760 mm
1 mm Hg = 1 torr
The standard atmospheric pressure
at sea level and 00C
= 760 mm Hg = 760 torr

10. COMMON UNITS OF PRESSURE
G A S L A W S
PRESSURE is the force exerted in a unit area.
The SI unit is Pa (pascal) = 1 Newton per square
meter
1 kilopascal = 1.01325 x 105 Pa
Blaise Pascal, a French
mathematician

11. COMMON UNITS OF PRESSURE
G A S L A W S

12. CHECKPOINT!!!
G A S L A W S
Why do mountain
climbers have
difficulty breathing
as they go higher up
the mountains?

13. OBJECTIVES:
B O Y L ‘ S
1. State Boyle’s law
2. Calculate changes in gas volume resulting
from pressure changes and vice versa
L
E
A W

14. B O Y L
A W
S
L
E ‘
Robert Boyle discovered the first of the simple gas laws,
now known as Boyle’s Law.
The pressure acting on the gas is the sum of the pressure
of the atmosphere.

15. B O Y L
A W
S
L
E ‘
EXPERIMENT PRESSURE (atm) VOLUME (mL) PRESSURE X VOLUME 1/P
1 0.5 1,200 600 2
2 1.0 600 600 1
3 2.0 300 600 0.5
4 3.0 200 600 0.333
5 4.0 150 600 0.25
6 5.0 120 600 0.2
7 6.0 100 600 0.167

16. B O Y L
A W
S
L
E ‘
EXPERIMENT PRESSURE (atm) VOLUME (mL) PRESSURE X VOLUME 1/P
1 0.5 1,200 600 2
2 1.0 600 600 1
3 2.0 300 600 0.5
4 3.0 200 600 0.333
5 4.0 150 600 0.25
6 5.0 120 600 0.2
7 6.0 100 600 0.167
PRESSURE
AND
VOLUME
VOLUME AND
RECIPROCAL
PRESSURE
Inverse relationship: when pressure
decreases, volume increases, and vice
versa, when temperature is constant
Direct relationship: when volume is
increasing/decreasing, reciprocal pressure
is also increasing/decreasing when
temperature is constant

17. B O Y L
A W
S
L
E ‘
It states that for a fixed amount of gas at constant temperature, volume is inversely
proportional to pressure.
It states that for a fixed amount of gas at constant temperature, volume is inversely
proportional to pressure.
𝑽 ∝
𝟏
𝑷
(𝒗, 𝑻 𝒄𝒐𝒏𝒔𝒕𝒂𝒏𝒕) 𝑽 = 𝑲(
𝟏
𝑷
)
𝑷𝑽 = 𝑲
𝑷𝟏𝑽𝟏 = 𝑲 𝑷𝟐𝑽𝟐 = 𝑲
𝑷𝟏𝑽𝟏 = 𝑲=𝑷𝟐𝑽𝟐

18. B O Y L
A W
S
L
E ‘
𝑷𝟏𝑽𝟏 = 𝑲=𝑷𝟐𝑽𝟐
A sample of a gas at 0.5 atm pressure and 250C
occupies a volume of 2.0 L. What pressure is
necessary to cause the gas to occupy 0.5 L at 250C?
ANALYZE PLAN CALCULATE

19. B O Y L
A W
S
L
E ‘
𝑷𝟏𝑽𝟏 = 𝑲=𝑷𝟐𝑽𝟐
A sample of a gas at 0.5 atm pressure and 250C occupies a volume of 2.0 L.
What pressure is necessary to cause the gas to occupy 0.5 L at 250C?
ANALYZE
P1 = 0.5 atm
V1 = 2.0 L
V2 = 0.5 L
P2 = ?
PLAN
Volume decreased.
Therefore, pressure
is expected to have
increased.
CALCULATE
𝑃2 =
𝑃1𝑉1
𝑉2
=
(0.5𝑎𝑡𝑚)(2.0 𝐿)
(0.5 𝐿)
=2.0 atm

20. B O Y L
A W
S
L
E ‘
𝑷𝟏𝑽𝟏 = 𝑲=𝑷𝟐𝑽𝟐
A sample of gas at 650 torr and 250C occupies a
volume of 400 mL. What volume will the gas occupy
at 900 torr and 250C?
ANALYZE PLAN CALCULATE
𝟐𝟖𝟗 𝒎𝑳

21. B O Y L
A W
S
L
E ‘
𝑷𝟏𝑽𝟏 = 𝑲=𝑷𝟐𝑽𝟐
What happens to the pressure of a gas in a closed
system if volume changes from 250 mL to 500 mL at
constant temperature?
ASSIGNMENT
What happens to a helium-filled balloon as it
continues to rise in the air? Does it drift out of Earth’s
atmosphere and end up in outer space?