OECD bibliometric indicators: Selected highlights, April 2024
Boyle's law (1).pptx
1.
2. PRAYER
Dear Lord and Father of all, thank you for
today.
Thank you for ways in which you provide for
us all.
For your protection and love we thank you.
Help us to focus our hearts and minds now
on what we are about to learn.
Inspire us by your eternal light as we
discover more about the world around us.
We ask all this in the name of Jesus.
Amen.
3. Mute your phone except when you
have the floor to talk.
Raise your hand virtually for
permission to speak.
Keep your camera on throughout
the discussion
Stay in a study place where there
are no distractions as we go on to
the lesson
7. 03
During inhalation, muscles increase the size of our thoracic (chest) cavity and
expand our lungs. This increases their volume, so pressure inside the lungs
decreases.
8. 03
Our lungs contracts and decreases the size of the chest cavity. This decreases the
volume, so pressure inside the lungs increases during exhalation.
11. a.) state the relationship between volume and
pressure of a gas at constant temperature;
b.) derive formula for Boyle’s Law;
c.) solve problems involving change in condition of
a gas using the equation for Boyle’s Law and
d.) cite applications of Boyle’s Law in real life
situation
17. Pressure increases when
volume decreases and
vice versa.
02. How do you describe the
relationship of pressure and
volume of a gas at constant
temperature?
18. 03. How do we express the
Boyle’s Law mathematically?
V ∝
1
𝑃
at constant temperature (k)
19. V ∝
1
𝑃
at constant temperature (k)
Thus, VP=k
Where: 𝑃1= initial pressure
𝑉1= initial volume
𝑃2= final pressure
𝑉2= final volume
𝑃1𝑉1= 𝑃2𝑉2
24. SAMPLE PROBLEM #1
The inflated balloon that slipped from
the hand of Kyla has a volume of
0.50 L at sea level (1.0 atm) and it
reached a height of approximately 8
km where the atmospheric pressure
is approximately 0.33 atm. Assuming
that the temperature is constant,
compute for the final volume of the
balloon.
Given:
Solution:
25. SAMPLE PROBLEM #2
The gas in the balloon has
a 4L at 1.44 atm. The
balloon is released into the
atmosphere, and the gas in
it expands to a volume of
8L. What is the pressure (in
torr) on the balloon at the
new volume?
Given:
Solution:
26. 01
A gas occupies 11.2 mL
at 0.860 atm. What is the
pressure if the volume
becomes 15.0 mL?
02
Two hundred milliliter (200
mL) of gas is contained in a
vessel under a pressure of
800 mmHg. What will be the
new volume (in L) of the gas
if the pressure is changed to
1000 mmHg? Assume that
the temperature remains
constant.
28. Given:
𝑽𝟏 = 𝟐𝟎𝟎 𝒎𝐋 𝑽𝟐 =?
𝑷𝟏= 𝟖𝟎𝟎 𝐦𝐦𝐇𝐠 𝑷𝟐=1000 mmHg
Solution:
𝑉2= 𝑃2𝑉2
𝑃1
𝑉2=(200 mL) (800 mm Hg)
1000 mm Hg
𝑽𝟐= 160 mL x
𝟏 𝑳
𝟏𝟎𝟎𝟎 𝒎𝑳
= 0.16 L
29. Boyle’s Law
(1)
formulated by
states that
The pressure (p) of a given
quantity of gas varies
___(2)____ with its volume (v)
at constant temperature.
In other words,
as the pressure ___(3)____, the
volume decreases. Conversely,
as pressure ___(4)____,
volume increases.
Mathematically written as (5)
Hence,
(6)
Where
(6)
𝑷𝟏
𝑽𝟏
(7)
𝑷𝟐
(8)
𝑽𝟐
(9)
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
30. Boyle’s Law
ROBERT BOYLE
formulated by
states that
The pressure (p) of a given
quantity of gas varies
___(2)____ with its volume (v)
at constant temperature.
In other words,
as the pressure ___(3)____, the
volume decreases. Conversely,
as pressure ___(4)____,
volume increases.
Mathematically written as (5)
Hence,
(6)
Where
(6)
𝑷𝟏
𝑽𝟏
(7)
𝑷𝟐
(8)
𝑽𝟐
(9)
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
31. Boyle’s Law
ROBERT BOYLE
formulated by
states that
The pressure (p) of a given
quantity of gas varies
inversely with its volume (v)
at constant temperature.
In other words,
as the pressure ___(3)____, the
volume decreases. Conversely,
as pressure ___(4)____,
volume increases.
Mathematically written as (5)
Hence,
(6)
Where
(6)
𝑷𝟏
𝑽𝟏
(7)
𝑷𝟐
(8)
𝑽𝟐
(9)
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
32. Boyle’s Law
ROBERT BOYLE
formulated by
states that
The pressure (p) of a given
quantity of gas varies
inversely with its volume (v)
at constant temperature.
In other words,
as the pressure increases, the
volume decreases. Conversely,
as pressure decreases, volume
increases.
Mathematically written as (5)
Hence,
(6)
Where
(6)
𝑷𝟏
𝑽𝟏
(7)
𝑷𝟐
(8)
𝑽𝟐
(9)
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
33. Boyle’s Law
ROBERT BOYLE
formulated by
states that
The pressure (p) of a given
quantity of gas varies
inversely with its volume (v)
at constant temperature.
In other words,
as the pressure increases, the
volume decreases. Conversely,
as pressure decreases, volume
increases.
Mathematically written as
Hence,
(6)
Where
(7)
𝑷𝟏
𝑽𝟏
(8)
𝑷𝟐
(9)
𝑽𝟐
(10)
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
34. Boyle’s Law
ROBERT BOYLE
formulated by
states that
The pressure (p) of a given
quantity of gas varies
inversely with its volume (v)
at constant temperature.
In other words,
as the pressure increases, the
volume decreases. Conversely,
as pressure decreases, volume
increases.
Mathematically written as
Hence,
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
Where
(7)
𝑷𝟏
𝑽𝟏
(8)
𝑷𝟐
(9)
𝑽𝟐
(10)
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
35. Boyle’s Law
ROBERT BOYLE
formulated by
states that
The pressure (p) of a given
quantity of gas varies
inversely with its volume (v)
at constant temperature.
In other words,
as the pressure increases, the
volume decreases. Conversely,
as pressure decreases, volume
increases.
Mathematically written as
Hence,
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
Where
𝑷𝟏
𝑽𝟏
(8)
𝑷𝟐
(9)
𝑽𝟐
(10)
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
36. Boyle’s Law
ROBERT BOYLE
formulated by
states that
The pressure (p) of a given
quantity of gas varies
inversely with its volume (v)
at constant temperature.
In other words,
as the pressure increases, the
volume decreases. Conversely,
as pressure decreases, volume
increases.
Mathematically written as
Hence,
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
Where
𝑷𝟏
𝑽𝟏
𝑷𝟐
(9)
𝑽𝟐
(10)
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
37. Boyle’s Law
ROBERT BOYLE
formulated by
states that
The pressure (p) of a given
quantity of gas varies
inversely with its volume (v)
at constant temperature.
In other words,
as the pressure increases, the
volume decreases. Conversely,
as pressure decreases, volume
increases.
Mathematically written as
Hence,
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
Where
𝑷𝟏
𝑽𝟏
𝑷𝟐
𝑽𝟐
(10)
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
38. Boyle’s Law
ROBERT BOYLE
formulated by
states that
The pressure (p) of a given
quantity of gas varies
inversely with its volume (v)
at constant temperature.
In other words,
as the pressure increases, the
volume decreases. Conversely,
as pressure decreases, volume
increases.
Mathematically written as
Hence,
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
Where
𝑷𝟏
𝑽𝟏
𝑷𝟐
𝑽𝟐
𝑷𝟏𝑽𝟏= 𝑷𝟐𝑽𝟐
42. A. Follow-up
1. A quantity of a gas confined has a volume of 30m³ at 800
torr. If the pressure of the gas is raised to 1000 torr, what would
be the new volume of the gas? The temperature remains constant.
2. Thirty cubic meters (30 m³) of gas in a large cylinder exerts
a pressure of 1.75 atm. Find the pressure the same gas
should exert for the volume to become 40 m³. Assume no change in
temperature.
B. Advance:
1. How is temperature and volume related at constant
pressure?
2. Cite some applications of Charle’s Law?
Reference: Science Quarter 4 – Module 1.2: Charles’ Law (Pg 1-16)
Editor's Notes
May we have Irish to lead the prayer for us before we’ll start the session.
How are you class? Is everyone doing fine? Did you take ur breakfast?
Before we start with our topic for today, please be reminded of the following rules as we go on with our topic.
This morning you will explore a new concept but before that may I ask everyone to take a deep breathe. Everybody, inhale then exhale. Inhale then exhale.
This pressure-volume relationship is also called as Boyle’s Law.
Today you will learn the relationship of pressure and volume of a gas a constant temperature.
For our objectives for today’s topic we have the following
For clearer understanding of the topic, let us have an activity entitled “Marvelous Balloon”
What do you call the law that is being demonstrated?
Who is the man behind this law?
The Boyle’s Law was first stated by Robert Boyle. He performed an experiment wherein he trapped a fixed amount of air in the J-tube, he changed the pressure and controlled the temperature and then he observed its effect to the volume of air inside the J-tube.
Based on the experiment, how are pressure and volume related?
From the given equation for Boyle’s law, what will be the formula if the unknown is initial volume?
If the problem is asking you to solve for the initial pressure, what formula or equation are you going to use?
What about if final pressure is unknown?
Any unit of pressure and volume may be employed. However, consistency of units must be observed.
Let’s apply the different formula with these sample problems.
A good place to start this problem is to write out the formula for Boyle's law and identify which variables you know and which remain to be found
Dividing both sides of the equation by V2 gives you:
Now substitute the known quantities into the equation and solve.
Are you ready to experience Boyle’s Law in action? Try to put the theory to practice. Prepare with you your pen, paper and calculator and solve this problem on your own. I will give you 2 minutes and after that, I will call one student to explain his or her work.
Using the terms provided below, complete the concept map.
Knowing the concept of pressure and volume, cite some applications of Boyle’s Law in our daily lives.