boyles law demo teaching

1. Rachel Ann C.
Ramilo
Teacher

4. USE THE PICTURES TO GUESS THE WORD.

9. ForPlaying
ThankYou

11. Procedure
1. Remove the needle of the syringe if there
is any.
Put a marshmallow inside the syringe.
2. Place your thumb over the end of the
syringe where
the needle is usually located. Holding
your thumb in
place, push in the plunger. Observe what
happens to the

12. What happen to the
marshmallows
when you push plunger of the
syringe?

13. What happened when the plunger
was pulled out?

15. VOLUME-PRESSURE
RELATIONSHIP

16. Boyle’s Law
Charles’ Law
Gay-Lussacs Law
Avogadro’s Law

17. Who do you think is
the proponent of
Boyle’s law?

18. Robert Boyle
Boyle’s Law was named after chemist
and physicist Robert Boyle,
who published the original law in
1662.

19. Boyle’s law states that the volume of a gas is
inversely proportional to its pressure (P)
at constant temperature (T).
In symbol; P∞ 1/V

20. Volume (V) Pressure (P) VxP
2.0 10.00
4.0 5.00
8.0 2.50
16.0 1.25
The table below shows volume and pressure data for a set
amount of gas at the constant temperature.

21. Volume (V) Pressure (P) VxP
2.0 10.00
4.0 5.00
8.0 2.50
16.0 1.25
The table below shows volume and pressure data for a set
amount of gas at the constant temperature.
20
20
20
20

22. Boyle’s
Law
PV=k
Therefore:
P1V1= k
P2V2= k
then ,
P1V1=P2V2

23. Based on the relationship of pressure and
volume, what do you think will happen to
the volume if pressure of a gas doubles?
Based also on the relationship of pressure
and volume, in what particular situation
where you can relate the concept of
pressure volume relationship?

24. A sample of nitrogen gas (N2) has a
volume of 12L and pressure of
760mmHg. When the gas is released, it
gives 32L of nitrogen. If the
temperature is the same, what is the
new pressure of hydrogen?
sample problem
1

25. Solution
;
GIVEN:
P1=
760mmHg
V1= 12L
V2 = 32L
P2 = ?
Derived the equation for
P2 using Boyle’s Law:
P1V1=P2V2
FORMULA:
P2= P1V1
V2
SOLUTION:
P2=
760mmHg(12L)
32L
P2 = 19,120
mmHg
32
P2 = 285
mmHg
The final pressure is 285
mmHgt

26. A gas tank holds 20L of
oxygen (O2) at a pressure of
15atm. How many liters will the
gas occupy if the pressure is
changed to 0.800atm at
constant temperature?
sample problem
2

27. Solution
;
GIVEN:
Given
P1= 15atm
V1= 20.0L
P2 =
0.800atm
V2 = ?
Derived the equation for
V2 using Boyle’s Law:
P1V1=P2V2
FORMULA:
V2= P1V1
P2
SOLUTION:
The final volume is
375L
V2= 15atm (20L)
0.800atm
V2 = 300L
0.800
V2
=
375L

29. 1. A 4.2L balloon holds air at 580torr.
If the balloon expands to 5.6L, what will
the pressure of the air inside become?
2. The volume of air in the marshmallows
blaster is 450ml. The pressure is 1.00
atm. If I decrease the volume to 50ml,
what will the new pressure be?

30. 3. A tank of nitrogen has a volume of
14.0 L and a pressure of 760.0 mm Hg.
Find the volume of the nitrogen when its
pressure is changed to 400.0 mm Hg while
the temperature is held constant.
4. A gas has a volume of 100
ml, when the pressure is 735
mmHg. How many milliliters will the
gas occupy at 700 mm Hg?

31. 1. A 4.2L balloon holds air at 580torr. If the balloon expands to 5.6L,
what will the pressure of the air inside become?
Given
P1= 580 torr
V1= 4.2L
P2= ?
V2=5.6L
Solution:
P2= 580torr (4.2
L)
5.6L
P2= 2,436torr
5.6
P2= 435 torr
Formula:
P1V1=P2V2
P2= P1V1
V2
The final pressure is
435 torr.

32. 2. The volume of air in the marshmallows blaster is 450ml. The pressure
is 1.00 atm. If I decrease the volume to 50ml, what will the new
pressure be?
Given
P1=
1.00atm
V1= 450ml
V2=50ml
P2= ?
Formula:
P1V1=P2V2
P2= P1V1
P2
Solution:
P2= 1.00atm
(450ml)
50ml
P2= 450
50
P2= 9.00 atm
The final pressure is
9.00atm

33. 3. A tank of nitrogen has a volume of 14.0 L and a pressure of 760.0
mm Hg. Find the volume of the nitrogen when its pressure is changed to
400.0 mm Hg while the temperature is held constant.
Given;
P1=760.0
mmHg
V1= 14.0 L.
P2= 400.0
mmHg
V2=?
Formula:
P1V1=P2V
2
V2= P1V1
P2
solution:
V2= 760.0 mmHg
(14.0 L.)
400.0 mmHg
V2= 10640 L.
400.0
V2= 26.6 L.
The final volume is
26.6 L.

34. 4. A gas has a volume of 100 ml, when the pressure is 735 mmHg.
How many milliliters will the gas occupy at 700 mm Hg?
Given;
P1=735
mmHg
V1= 100 ml
P2= 700
mmHg
V2=?
Formula:
P1V1=P2V
2
V2= P1V1
P2
Solution:
V2= 735 mmHg
(100ml)
700mmHg
V2= 73500 ml.
700
V2= 105 ml.
The final volume is
105 ml.

35. What does Boyle’s Law states?
What will happen if the pressure
increases?
What about if the volume
increases?

36. - If the pressure increases the
volume decreases.
- If the volume increases, the
pressure decreases.
- Boyle’s law states that the volume of a gas is
inversely proportional to its pressure (P) at constant
temperature (T).

37. Cite a real life
situation wherein the
concept of Boyles is
being applied.

38. You can observe a real-life
application of Boyle's Law when
you fill your bike tires with
air. When you pump air into
a tire, the gas molecules
inside the tire get compressed
and packed closer together.
This increases the pressure of
the gas, and it starts to
push against the walls of the
tire.

41. A. Multiple Choice: Choose the letter of the correct
answer.
___1. What law describes the relationship of the volume
of the gas to its pressure when mass and temperature
are held constant?
a. Boil’s Law c. Boyle’s Law
b. Boles’ Law d. Broil’s Law
_2. Who conceptualized the relationship between the volume
and
pressure of the gas that varies
inversely proportional to each other at constant
temperature and mass?
a. Robby Boyle c. Rob Boyle

42. ___3. In Boyle’s Law when the mass and temperature are
held constant, what happens to the volume if the pressure
increases?
a. Increase c. Decrease
b. Unchanged d. Became zero
___4. In contrast to no. 3 what happens to the volume
if the pressure decreases?
a. Increase c. Decrease
b. Unchanged d. Became zero
______5. Which of the following best describe the concept of Boyle’s
Law?
a. Hot air balloon c. Pressure Cooker

43. B. Direction: Solve the following. (Show your
solution)
1. A gas occupies 25.3 mL at a pressure of
790.5 mm Hg. Determine the volume if the pressure
is reduced to 0.804 atm.
2. Convert 77.0 L at 18.0 mm of Hg to its
new volume at standard pressure.
3. 500.0 mL of a gas is collected at 745.0 mm

44. A. Give two (2) good and bad effects of
using
Boyle’s Law in our daily living.
B. Answer the following question;
1. What is Charles law?
2. What are the variables involve
in Charles law?