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Science Activity Sheet
Quarter 4 – MELC 1
Weeks 1-2
Gas Laws
REGION VI – WESTERN VISAYAS
Science 10
Activity Sheet No. 1: Gas Laws
First Edition, 2021
Published in the Philippines
By the Department of Education
Region 6 – Western Visayas
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Development
Elena
P. Gonzaga,Team of Science Activity Sheet
Donald
T.
Writer: Melvin B. Medina
Genine
Rovel T. Pastias
R.
Editors: Rochelle
, Ma. Concepcion G. Pagcaliwagan
Salcedo,
Illustrator: Moonyeen
Melvin B. C.
Medina
Rivera,
Anita
S. Grande
Layout Artist:
Jennie H.
Gubalane,
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L.
School Division
Quality Assurance Team
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T. Pastias
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L. Lopez,
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Fatima A. Cordero
Grace B. Jungco
Ana Lee C. Bartolo
Division of La Carlota City Management Team
Neri Anne M. Alibuyog,
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Ana Lee C. Bartolo
Ma. Concepcion G. Pagcaliwagan
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Regional Management Team
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Donald T. Genine
Anita S. Gubalane
Moonyeen C. Rivera,
Minda L. Soldevilla
Joseph M. Pagalaran
Daisy L. Lopez
Introductory Message
Welcome to Science 10!
This Learning Activity Sheet is a product of the collaborative efforts of
the Schools Division Office of La Carlota City and DepEd Regional Office VI – Western
Visayas through the Curriculum and Learning Management Division (CLMD). This was
developed to guide the learning facilitators (teachers, parents and responsible adults)
in helping the learners meet the standards set by the K to 12 Basic Education
Curriculum.
This Learning Activity Sheet is a self-directed instructional material aimed to
guide the learners in accomplishing activities at their own pace and time using the
contextualized resources in the community. This will also assist the learners in
acquiring the lifelong learning skills, knowledge and attitudes for productivity and
employment.
For the learning facilitator:
This Science 10 Activity Sheet will help you facilitate the teaching-learning
activities for the specified Most Essential Learning Competency (MELC) with minimal
or no face-to-face encounter between the teacher and the learner. This is made
available to the learners with the references/links to ease independent learning.
For the learner:
This Science 10 Activity Sheet was developed to help you continue learning
even if you are not in school. This learning material provides you with meaningful and
engaging activities for independent learning. Being an active learner, carefully read
and understand the instructions then perform the activities and answer the
assessments. This will be returned to your school and teacher on the agreed schedule.
Name of Learner: _________________________________________________________
Grade and Section: _____________________________ Date: ____________________
SCIENCE 10 ACTIVITY SHEET No. 1
Gas Laws
I. Learning Competency with Code
Investigate the relationship between volume and pressure at constant
temperature of a gas; volume and temperature at constant pressure of a gas
and explains these relationships using the kinetic molecular theory (S10MTIV-a-b-21).
II. Background Information for Learners
This learning activity offers interesting discussion about gases. You are
given the chance to get to know important concepts and ideas that will make
you appreciate the properties and the behavior of gases.
Most gases are invisible to your naked eye. You can name as many solids
and liquids that you can see around but not gases. You can only name a very
few colored ones like the black smoke produced by vehicles or the ones you
see in your kitchen when you cook with firewood or charcoal. Invisible gases
are present everywhere. They are in a clear bottle that seems to be empty, in
the production of food by the plants during photosynthesis, and even in
playing your favorite sports. Can you ride your bicycle if its wheels are not
sufficiently filled with air or gas? Your very existence requires the presence of
invisible gases. You inhale oxygen and exhale carbon dioxide during the
process of respiration. Can you survive here on earth without these gases?
In this learning activity, you will learn the different properties of gases
and how these properties are related to one another. Furthermore, after going
through the activities provided, you will explain the relationships that exist
between the properties of gases in terms of the Kinetic Molecular Theory.
III. Accompanying DepEd Textbook
Department of Education. (2015). K-12 Basic Education Curriculum,
Science 10 Learner’s Material (pp 171-182). Pasig City, Philippines
Department of Education. (2015). K-12 Basic Education Curriculum,
Science 10 Teacher’s Guide (pp 48). Pasig City, Philippines
IV. Activity Proper
ACTIVITY 1
Properties of Gases
Study the situations below and answer the questions that follow.
Write the answer on your answer sheet.
Situation 1.
The mass of a deflated balloon was measured using a digital balance.
Such balloon was later inflated and place again on the digital balance to
determine its mass. Data were gathered and indicated in the table below.
Study the table and answer the questions that follow.
Table 1. Comparison of the mass of inflated and deflated balloon.
Trial
Mass of the deflated
Mass of the inflated
balloon in grams
balloon in grams
1
3.46
13.21
2
3.48
13.76
3
3.49
15.01
Questions.
1. Which is heavier, the deflated or inflated balloon? Why?
___________________________________________________________________________
2. What can you infer from the data presented in the table?
__________________________________________________________________________
Situation 2.
An approximately 40 mL of water was placed in a graduated cylinder.
It was then added with cooking oil up to 60 mL. After a while the oil float on
top of the water. Later, the tip of syringe (with its plunger pulled up) was
dipped in the mixture until it reaches the water portion. The plunger was
pushed down, and the volume of the mixture was again recoded as shown in
Table 2.
Table 2.
Trial
Volume of water plus
Total volume when air
oil
was introduced
1
2
3
60 mL
60 mL
60 mL
87 mL
90 mL
91 mL
Questions.
1. What happens to the volume of water and oil mixture when air was
introduced?
________________________________________________________________________
2. What does it indicate?
_____________________________________________________________________
Situation 3.
A 150 mL water was placed in a beaker. Using a thermometer, the initial
temperature of the air above the water was determined. The beaker is then
filled with ice cubes and after 5 minutes, the temperature of the air above it
was measured and recorded. Finally, the beaker was placed on a tripod over
an alcohol lamp. It was heated until it boils, then the temperature of air just
above the water was measured. The data gathered in this activity are indicated
in the Table 3 below.
Table 3. Temperature of air
Trial
Initial
temperature
air
1
23°C
2
23°C
3
23°C
Temperature of Temperature of
of air above iced air above the
water
boiling water
14°C
85°C
15°C
88°C
14°C
92°C
Question.
1. Is there a difference in the temperature of air in the three set-ups? If yes,
explain what cause/s the difference.
______________________________________________________________________
Situation 4.
An inflated balloon was placed in the mouth of an Erlenmeyer flask with
hot water. After a few minutes, the balloon inflated. In another case, a deflated
balloon was placed in the mouth of an Erlenmeyer flask with water. The flask
was heated over an alcohol lamp. After a while, the balloon starts to inflate
and changes its size and shape.
Questions.
1. What cause/s the changes in the size and shape of inflated balloon
when place in an Erlenmeyer flask with hot water?
________________________________________________________________________
2. What cause/s the balloon in the Erlenmeyer with water to inflate and
changed its size and shape when the flask was heated?
________________________________________________________________________
After knowing that gases have mass, volume, temperature, and pressure,
it’s a must for you to familiarize with the units being used to express these
measurable properties of gases.
The table below shows the common units and some of their interconversions.
Table 1: Common Units for
Variable
SI Unit
Volume
cubic meter (m3)
cubic decimeter(m3)
cubic centimeter(m3)
Pressure
Pascal (Pa)
Pressure and Volume
Metric Unit
English Unit
liter (L)
Quart (qt)
milliliter (mL)
Gallon (gal)
atmosphere
torr
(atm)
lb/in2 psi
millimeters of
mercury (mm
Hg)
centimeters of
mercury (cm Hg)
Volume units and their equivalents:
1 mL = 1 cm3; 1 L = 1 dm3 ;1 m3 = 1000 L
Pressure units and their equivalents:
1 atm = 760 mm Hg = 76 cm Hg = 760 torr = 101325 Pa = 14.6956 psi = 9.81
N/cm2
Temperature units and their equivalents:
0˚C = 273.15 K; 0˚C = 32˚F
These units of measure will be utilized as you go along with the
discussions on gases. The measurable properties of gases are interrelated and
can be modeled mathematically.
Now, you will investigate the relationship between the volume and
pressure of a confined gas at constant pressure.
ACTIVITY 2
Volume-Pressure Relationship in Gases
Have you observed how the balloon expands and gets hard when you
blow air on it? Have you also observed what happens when you squeezed an
inflated balloon? This activity gives a quantitative treatment of the
relationship between volume and pressure in gases.
What you need
Plastic or syringe
Graphing paper
What you have to do
A. Qualitative Treatment of Volume-Pressure Relationship
1. Observe the qualitative relationship between gas volume and pressure
at constant temperature. Follow these steps:
a. Fill a syringe with air by pulling the plunger up.
b. Press your finger against the end of the tip of the syringe in order to
trap the air.
c. Push the plunger in. Try again but press harder this time.
Directions. Answer the following questions. Write the answer on your answer
sheet.
1. What have you observed?
___________________________________________________________________________
2. Is the trapped air in the syringe affected by the added pressure as you press
down the plunger with minimal force?
___________________________________________________________________________
3. How do you relate the pressure (ex., applied force) to the volume or
compressibility of air in the syringe?
___________________________________________________________________________
B. Quantitative Treatment of Volume-Pressure Relationship
A syringe having a diameter of 1.5 cm was filled with a volume of air
as shown in Column A in the table below. A force that acts on the volume of
air was also determined and are indicated in Column B.
Directions: Copy and complete the data Table 1.1. Compute for Pressure
(Column C) Total Pressure (Column D) P x V (Column E) Pt x V (Column F)
and P/V (Column G). Item number 1 is done for you. Write the answer on
your answer sheet.
Table 1.1 Data for deriving pressure-volume relationship
Volume
(V) of air
in
syringe
(cm3)
Pressure (P)
(force/area of
plunger)
(N/cm2)
(A)
Force (F)
(weight of
plunger) +
weight
added to
plunger, (N)
(B)
4.9
0.6
0.34
4.4
4.0
3.6
3.4
2.6
4.6
6.8
8.8
(C= B/1.77)
Total
pressure (Pt)
(Pt =P+)
atmospheric
pressure )
(N/cm2)
(D= 10 +C)
10+0.34=
10.34
PxV
Pt x V
P/V
(E=AxC)
(F=AxD)
(G=C/A)
1.67
50.47
0.06
Since the inside diameter (d) of the syringe is given, you can compute
the area of the plunger circular cross section. The formula for finding the area
of a circle is
A= πr2, where r is radius
Since d = 1.5 cm and d= 2r, A = π (d/2)2. Upon substitution to the
equation, you can obtain A = 1.77 cm2
Step 1
Compute the pressure (P) using the equation P = F/A. Record your answers
in the Column C of Table 1.1. For the given set of data in the table, pressure
is computed a:
P = 0.6N/1.77 cm2 = 0.34 N/ cm2.
Step 2:
The atmosphere also exerts pressure on the plunger. The total pressure
(Column C) on the air in the syringe is the sum of the atmospheric pressure,
which is 10 N/cm2 at sea level and the pressure due to force (F) applied. In
the first set of data, the total pressure is computed as
Pt = 0.34 N/cm2 + 10 N/cm2 = 10.34 N/cm2
Step 3
Plot a graph with the pressure at the y axis and volume at the x axis. Do this
in your answer sheet.
Directions. Answer the following. Write the answer on your answer sheet.
1. What happened to the volume of the syringe as the set of weights is added
on top of it?
___________________________________________________________________________
2. What happened to the pressure on the syringe when the set of weights is
added?
___________________________________________________________________________
3. Describe the graph.
___________________________________________________________________________
4. What is the relationship between volume and pressure of gases as
indicated in the graph?
___________________________________________________________________________
The relationship between the volume and pressure of gases at constant
temperature is known as Boyle’s law. The law states that the volume V of a
sample of gas changes inversely with the pressure P of the gas as long as the
temperature T and the amount of gas n remain constant. This means that if
the volume is doubled, the pressure will be reduced by one-half.
Boyle’s law equation can be expressed as:
Vα
1
at constant T and n
P
Where:
V = volume, P = pressure, T = temperature and n = amount of the gas.
The volume of a gas is inversely proportional to its pressure, if
temperature and amount of a gas are held constant. Take a look at the
equation again and try to change the proportionality sign (α) with the equal
sign (=).
1
Vα
at constant (k)
P
V=
k
Thus, k = VP
P
P1V1 = P2V2
(Boyle’s Law Equation)
Sample Problem
The inflated balloon that slipped from the hand of Renn 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.
Initial Conditions
V1= 0.50 L
P1= 1.00 atm
Equation:
P1V1
V2 =
P2
Solution:
P1V1
V2 =
P2
(1.0 atm) (0.50 L)
V2 =
0.33 atm
0.5 L
V2 =
= 1.5 L
0.33
Final Conditions
V2=?
P2= 0.33 atm
ACTIVITY 3
Boyle’s Law Problem
Directions: Read and understand each problem. Use Boyle’s law to solve the
problem by writing the given, equation and solution. Box your final answer.
Write the answer on your answer sheet.
1. A scuba diver needs a diving tank in order to provide breathing gas while
he is underwater. How much pressure is needed for 6.00 liters of gas at 1.01
atmospheric pressure to be compressed in a 3.00-liter cylinder?
ACTIVITY 4
Volume-Temperature at Constant Pressure
What relationship exists between the volume and temperature of gas?
What you need
1 rubber balloon 1 small basin
tape measure
tap water
hot water
ice
What you have to do
1. Prepare 1 small basin.
2. Inflate a balloon.
3. Measure the circumference of the balloon
using a tape measure.
4. Fill half of the basin with 1 L hot water.
5. Submerged the inflated balloon in hot water
for 5 minutes by pushing down with your
hands. Then measure again its circumference.
Record your data. Do the same for second and
third trial.
Warning: Exercise caution when performing this activity.
6. Repeat procedures 2-5 using tap water and cold water.
7. Record the results in table 1.2
Table 1.2 Data on Determining the Size of the Balloon at Different
Temperatures
Set-up
Temperature Average Circumference of the Balloon (cm)
Description
Trial 1
Trial 2
Trial 3
Hot water
hot
Tap water
warm
Cold water
cold
Directions. Answer the following questions. Write the answer on your answer
sheet.
1. What happens to the size of the balloon as the temperature decreases?
___________________________________________________________________________
2. How does the change in the temperature relate to the volume of gas in the
balloon?
___________________________________________________________________________
The volume - temperature relationship in gases (k = V/T) was
determined by and named after Jacques Charles. Charles’ Law states that at
constant pressure, the volume of a fixed amount of gas is directly proportional
to the Kelvin (K) temperature.
Mathematically, Charles’ Law can be expressed as:
V α T at constant P
Where: V = volume and T = temperature expressed in Kelvin
Kelvin is the basic unit for measuring temperature in the International
System (SI). “It denotes the absolute temperature scale whereby 0K or
absolute zero is defined as the temperature when molecules will have the
lowest energy.
Removing the proportionality symbol (α) and using the equality sign
(=) the equation will be as follows:
𝐕
V = k T or
𝒌=
𝐓
Whereas, V1 is the initial volume and V2 is the final volume T1 is the
initial temperature and T2 is the final temperature. If the volumetemperature ratios are the same in the initial and final conditions, then you
will arrive at this equation:
V1
=
T1
V2
(Charles’ Law Equation)
T2
Directions: Copy and complete the table with the necessary information on
your answer sheet. Then, plot the data from Table 1.3 in a graph by placing
the volume in the y axis and temperature at Kelvin scale in the x axis.
Trial
1
2
3
4
Table 1.3 Data on Volume-Temperature Relationship
Volume Reading (ml)
Temperature (oC)
Temperature (K)
25
30
35
40
2
57
102
152
Note: To convert °C to K, use this formula: K = °C + 273.15
Example: 5 °C = K, K = °C + 273.15, K = 5+ 273.15 = 278.15 K
Directions. Answer the following questions. Write the answer on your answer
sheet.
1. What happens to the temperature when the volume increases?
___________________________________________________________________________
2. Describe the graph.
___________________________________________________________________________
3. What is the relationship between volume and temperature of gases at
constant pressure?
___________________________________________________________________________
Apply Charles’ Law in solving problems related to volume- temperature
relationship in gases.
Sample Problem:
An inflated balloon with a volume of 0.75 L at 30°C was placed inside the
freezer where the temperature is -10°C. Find out what will happen to the
volume of the balloon if the pressure remains constant. Support your
answer with computation.
Initial Conditions
V1= 0.75L
T1= 30 0C =303K
Final Conditions
V2=?
T2= -10 0C =263 K
Equation:
V2 =
V1T2
T1
Solution:
V2 =
V2 =
V1T2
T1
(0.75 L) (263. K)
L)
V2 =
303. K
197.25 L
303
= 0.65 L
Activity 5
Solving Charles Law Problem
Directions: Read and understand each problem. Use Charles law to solve the
problem by writing the given, equation and solution. Box your final answer.
Write the answer on your answer sheet.
1. A cylinder with a movable piston contains
250 cm3 air at 10°C. If the pressure is kept constant, at what temperature
would you expect the volume to be 150 cm3?
Activity 6
Kinetic Molecular Theory
The Kinetic Molecular Theory (KMT) explains the properties of gases and
describes the behavior of gases. It states that:
1. Gases are composed of molecules. The distances
from one molecule to another molecule are far greater
than the molecules’ dimensions. These molecules can
be considered as spherical bodies which possess
negligible mass and volume.
Figure 1. Molecules of Gases
2. Gas molecules are always in constant random motion
and they frequently collide with one another and with
the walls of the container. Collision among molecules
are perfectly elastic, that is, energy may transfer from
molecule to molecule as the result of collision but the
total energy of all the molecules in the system remains
the same/constant.
3. There is a neither attractive nor repulsive force
between or among gas molecules.
4. Movement of gas molecules is affected by
Figure 2. Molecules of Gases in
Random Motion
temperature. The molecules move faster as the
Images are taken from Science10
temperature increases. This is due to heat that is
Learner’s Module
converted to KE energy of molecules. As the
molecules absorb more KE, they move faster and
bump the walls of the container causing it to expand, the material is elastic.
Activity 7
Directions. Answer the following questions on your answer sheet.
1. How do you explain the relationship of volume and pressure using the
Kinetic Molecular Theory?
_____________________________________________________________________
2. How do you explain the relationship of volume and temperature using
the Kinetic Molecular Theory?
____________________________________________________________________
Activity 2
A
1. The plunger does not move downward if the other end is closed.
2. No, a minimal force seems to have a very small effect on the plunger as it is
being pressed down.
3. The volume of air decreases as pressure increases.
B
Table 1.1 Data for deriving pressure-volume relationship
PxV
Pt x V
Pressure (P)
Total
pressure (Pt)
10.3
1.47
50
11.5
6.6
50
12.6
10.4
50
13.8
13.7
50
15.0
17.0
50
0.3
1.5
2.6
3.8
5.0
P/V
2.10
2.6
3.15
3.83
4.4
1. The volume decreases.
2. The pressure increases.
3. The recorded volume must be decreasing while the recorded pressure must be
increasing. Therefore, when a line graph of gas’ volume vs. its pressure is plotted,
with the pressure on the y axis and the volume on the x axis.
4. Inversely proportional.
Activity 1
Situation 1
1. Inflated balloon is heavier. The difference in the mass is due to the
addition of gas,
2. Gases like solids and liquids have mass too.
Situation 2
1. The volume increases
2. Gases have volume too.
Situation 3
1. Yes, Heat flows from the surroundings or vice versa. If the water is
cooled, the surrounding air also gets cooled. Conversely, if the
water is hot, the surrounding air also get hot.
Situation 4.
1. Heat flows. The heat from water is transferred to the air above it. As
the air gets heated, its molecules become excited and push the
walls of the balloon making changes in the size and shape.
2. As the water is heated until it boils, water vapors are produced. The
water vapors are warm and warm air goes up. In the setup the war
air goes to the balloon making it inflated. The more water vapor is
produced, the bigger the size of the balloon.
VI. Answer Key
1. What are some of the daily situations and activities observed at home
and the community that involves the properties of gases? Cite
examples.
V. Reflection
Activity 4
Table 1.2 Data on Determining the Size of the Balloon
Answers may vary.
1. The size of the balloon decreases.
2. As temperature decreases, the volume of the gas decreases.
Table 1.3 Data on Volume-Temperature Relationship
1. 275 K
2. 330 K
3. 375 K
4. 425 K
1. The temperature increases when the volume increases.
2. The graph is increasing.
3. Directly proportional.
Activity 5
1. Final temperature = 169.8K
Activity 6.
1. Attraction between gas particles.
2. The particles of a gas move rapidly.
3. Gas particles move at random motion with no attractive forces between
them.
Activity 7
1. According to Kinetic molecular theory, the molecules of gas are in
continuous motion. When the volume is less, collision is greater and
pressure between molecules increases.
2. According to Kinetic Molecular Theory, an increase in temperature
will increase the average kinetic energy of the molecules. At a higher
temperature, the pressure of a container is increased due to the increase
in the number of times gas molecules strike the container walls.
Graph
Activity 3
1. Final Pressure = 2.02 atmosphere