This is the instruction sheet for my MYP year 4 chemistry unit on thermal energy. It's a Vernier lab, which means it requires proprietary probes from the Vernier company. I have adapted the company's original document to highlight key steps for my students.
las características de la impetratoria, las escalas termométricas, asi como las variaciones en los estados de la materia que incluyen la dilatación y la cantidad de calor existente
Molecular Weight Determination by Freezing point depressionPicasa_10
It describes an experiment to determine Molecular weight of an unknown compound from a list of known compounds by Freezing point depression method. Further, this experiment was extended to compare the rate of freezing and rate of melting of ionic (NaCl) and covalent (urea) compounds.
Molarity vs Molality What is molarity? Molarity is also known as molar concentration, it is the ratio of moles of substance to volume in liter. Where mole is weight in gram divided by molecular weight. Molarity is chemistry terminology. Molarity... read more at https://chemistrynotesinfo.com/molarity-vs-molality/
las características de la impetratoria, las escalas termométricas, asi como las variaciones en los estados de la materia que incluyen la dilatación y la cantidad de calor existente
Molecular Weight Determination by Freezing point depressionPicasa_10
It describes an experiment to determine Molecular weight of an unknown compound from a list of known compounds by Freezing point depression method. Further, this experiment was extended to compare the rate of freezing and rate of melting of ionic (NaCl) and covalent (urea) compounds.
Molarity vs Molality What is molarity? Molarity is also known as molar concentration, it is the ratio of moles of substance to volume in liter. Where mole is weight in gram divided by molecular weight. Molarity is chemistry terminology. Molarity... read more at https://chemistrynotesinfo.com/molarity-vs-molality/
Some problems for calculating net primary productivity (NPP), gross primary productivity (GPP), and respiration (R) rates from given data. Aligned with the IB Environmental Systems and Societies course.
Some problems for calculating net primary productivity (NPP), gross primary productivity (GPP), and respiration (R) rates from given data. Aligned with the IB Environmental Systems and Societies course.
BC Chemistry 162 Laboratory Manual Experiment 6 Vapor Press.docxrosemaryralphs52525
BC Chemistry 162 Laboratory Manual
Experiment 6: Vapor Pressure of Liquids
- 1 -
Experiment 6: Vapor Pressure of Liquids
Background
Liquids contain molecules that have different kinetic energies (due to different velocities). Some of the
faster liquid molecules have enough kinetic energy to vaporize. At the same time, some of the slower
vapor molecules condense into liquid. In an open container, the rate of vaporization will be greater than
the rate of condensation—hence, the liquid will eventually evaporate. In a sealed flask, however, there
will be a point in which equilibrium is reached between the rate of vaporization and the rate of
condensation. To the eye, it seems that the liquid doesn’t change at equilibrium. But at the microscopic
level a vapor molecule enters the liquid phase for every liquid molecule that enters the gas phase.
The total pressure in the sealed flask is due to the vaporized liquid plus air molecules present in the flask:
Ptotal = Pvapor + Pair (1)
In this experiment, you will investigate the relationship between
the vapor pressure of a liquid and its temperature. Pressure and
temperature data will be collected using a gas pressure sensor and
a temperature probe (Figure 1). Vapor pressures will be
determined by subtracting atmospheric pressure from the total
pressure.
The flask will be placed in water baths of different temperatures to
determine the effect of temperature on vapor pressure. You will
measure the vapor pressure of methanol and ethanol and
determine the enthalpy (heat) of vaporization for each liquid.
Objectives
In this experiment, you will
Investigate the relationship between the vapor pressure of a liquid and its temperature.
Compare the vapor pressure of two different liquids at the same temperature.
Use pressure‐temperature data and the Clausius‐Clapeyron equation to determine the heat of
vaporization for each liquid.
Caution!
The alcohols used in this experiment are flammable and poisonous. Avoid inhaling their vapors. Avoid
contacting them with your skin or clothing. Be sure there are no open flames in the lab during this
experiment. Notify your teacher immediately if an accident occurs.
Procedure
1. Wear goggles! You will work in pairs for this lab, but you may share water baths with your table.
2. Prepare four water baths: 20 to 25°C (use room temperature water), 30 to 35°C, 40 to 45°C, and 50 to
55°C. You should also have some hot water on a hot plate on reserve.
3. Obtain a temperature probe and gas pressure sensor. The sensor comes with a
rubber‐stopper assembly (Figure 2). The stopper has three holes, one of which
is closed. Make sure your tubing and valve are not inserted in the closed hole.
Insert the rubber‐stopper assembly into a 125 mL Erlenmeyer flask.
Important: Twist the stopper into the neck of the flask to ensure a tight
fit.
Figure 1
Figure 2
BC Ch.
Bellevue College Chemistry 162 1 Empirical Gas La.docxtaitcandie
Bellevue College | Chemistry 162
1
Empirical Gas Laws (Parts 1 and 2)
Pressure-volume and pressure-temperature relationships in gases
Some of the earliest experiments in chemistry and physics involved the study of gases. The invention
of the barometer and improved thermometers in the 17th century permitted the measurement of
macroscopic properties such as temperature, pressure, and volume. Scientific laws were developed to
describe the relationships between these properties. These laws allowed the prediction of how gases
behave under certain conditions, but an explanation or model of how gases operate on a microscopic
level was yet to be discovered.
After Dalton’s atomic theory was proposed in the early 1800’s (that matter was composed of atoms) a
framework for visualizing the motion of these particles followed. The kinetic molecular theory,
developed by Maxwell and Boltzmann in the mid 19th century, describes gas molecules in constant
random motion. Molecules collide resulting in changes in their velocities. These collisions exert
pressure against the container walls. The frequency of collisions and the speed distribution of these
molecules depend on the temperature and volume of the container. Hence, the pressure of a gas is
affected by changes in temperature and volume.
You may already think that the relationships between pressure, volume, temperature, and number of
gas molecules are intuitive, based on your ability to visualize molecular motion and a basic
understanding of the kinetic theory. The simple experiments that follow will allow you the
opportunity to confirm these relationships empirically, in a qualitative and quantitative manner. In
essence, you will play the role of a 17th century scientist (with some 21st century tools!) and discover
the laws for yourself—laws and constants that are still in use today.
In this experiment, you will:
Determine the relationship between the volume of a gas and its pressure (Part 1).
Determine the relationship between the temperature of a gas and its pressure (Part 2).
Figure 1.
The Kinetic Theory considers
gas molecules as particles that
collide in random motion.
Bellevue College | Chemistry 162
2
Note: If you are doing Part 3 to determine the value of
the Universal Gas Constant, R in the same period as Parts 1
and 2, you should get Part 3 started first.
Part 1: Pressure-Volume Relationship of Gases
In Part 1 you will use a gas pressure sensor and a gas syringe to measure the pressure of an air sample
at several different volumes to determine the relationship between the pressure and volume of air at
constant temperature.
Figure 2
Procedure
1. a. Plug the gas pressure sensor into channel 1 of the computer interface.
b. With the 20 mL syringe disconnected from the gas pressure sensor, move the piston of the
syringe until the front edge of the inside black ring (indic.
LabQuest 7 Chemistry with Vernier 7 - 1 Pressure.docxMARRY7
LabQuest
7
Chemistry with Vernier 7 - 1
Pressure - Temperature
Relationship in Gases
Gases are made up of molecules that are in constant motion and exert pressure when they collide
with the walls of their container. The velocity and the number of collisions of these molecules are
affected when the temperature of the gas increases or decreases. In this experiment, you will
study the relationship between the temperature of a gas sample and the pressure it exerts. Using
the apparatus shown in Figure 1, you will place an Erlenmeyer flask containing an air sample in
four water baths of varying temperature. Pressure will be monitored with a Pressure Sensor and
temperature will be monitored using a Temperature Probe. The volume of the gas sample and the
number of molecules it contains will be kept constant. Pressure and temperature data pairs will
be collected during the experiment and then analyzed. From the data and graph, you will
determine what kind of mathematical relationship exists between the pressure and absolute
temperature of a confined gas. You may also do the extension exercise and use your data to find a
value for absolute zero on the Celsius temperature scale.
OBJECTIVES
In this experiment, you will
Study the relationship between the temperature of a gas sample and the pressure it exerts.
Determine from the data and graph, the mathematical relationship between pressure and
absolute temperature of a confined gas.
Find a value for absolute zero on the Celsius temperature scale.
Figure 1
MATERIALS
LabQuest plastic tubing with two connectors
LabQuest App 125 mL Erlenmeyer flask
Vernier Gas Pressure Sensor rubber stopper assembly
Temperature Probe ring stand and utility clamp
ice two 600 mL beakers
hot plate glove or cloth
beaker tongs
LabQuest 7
7 - 2 Chemistry with Vernier
PROCEDURE
1. Obtain and wear goggles.
2. Prepare a hot-water bath. Put about 400 mL of hot tap water into a 600 mL beaker and place
it on a hot plate. Turn the hot plate to a high setting. NOTE: Submerge Erlenmeyer flask to
neck to ensure that the water does not overflow. See Figure 3.
3. Prepare an ice-water bath. Fill a second 600 mL beaker with ice, ~ 1/3 full. Add cold tap
water to fill to the 400 mL mark.
4. Prepare the Temperature Probe and Gas Pressure Sensor for data collection.
a. Connect the Gas Pressure Sensor to Channel 1 of LabQuest and the
Temperature Probe to Channel 2. Choose New from the File menu.
If you have older sensors that do not auto-ID, manually set up the
sensors.
b. Obtain a rubber-stopper assembly with a piece of heavy-wall plastic
tubing connected to one of its two valves. Attach the connector at
the free end of the plastic tubing to the open stem of the Gas
Pressure Sensor with a clockwise turn. Leave its two-way valve on
the rubber stopper open (lined up with the valve stem as shown in Figure 2) until Step 4d.
c. Insert the rubber-stopper assembly ...
boyle's law thermodynamics lab Boyle’s law, also called Mariotte’s law, a relation concerning the compression and expansion of a gas at constant temperature. This empirical relation, formulated by the physicist Robert Boyle in 1662, states that the pressure (p) of a given quantity of gas varies inversely with its volume (v) at constant temperature; i.e., in equation form, pv = k, a constant. The relationship was also discovered by the French physicist Edme Mariotte (1676). ake a large piston or sealed syringe and stand it on end, then place an increasing number of objects on top. As the pressure grows, the volume of the air inside will decrease—these quantities are inversely proportional. However, the standard international unit for pressure is the Pascal. The English scientist Robert Boyle performed a series of experiments involving pressure and, in 1662, arrived at a general law—that the volume of a gas varies inversely with pressure.
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Molecular Weight of an Ideal Gas by the Dumas Method
Objectives:
1. In this experiment we will determine the molecular weight of air and CO2 by measuring P, T, V and weight of a gas sample.
2. You will become familiar with how experimental errors in several measurements combine to give the error in an overall calculated result.
3. You will also become familiar with the routine operation of a vacuum rack.
4. You will refine your lab report writing skills.
Introduction:
In this first experiment, you will determine the molecular weight of a gas by the Dumas method. In the Dumas method, the density of a gas or volatile liquid is determined at a known pressure and temperature. Using the ideal gas law, the molecular mass of the substance can be calculated:
where d is density, R is gas constant, T is temperature, P is pressure and M is molar mass of the gas.
To determine the density of the gas, both mass and volume will be measured independently. A glass bulb is evacuated and filled with the test gas. The difference in the mass of the filled vs. evacuated bulb will give you the mass of the gas. The volume of the bulb is determined by measuring the amount of water required to fill the bulb.
Buoyancy Correction:
In this experiment we are measuring the mass of a small volume of gas by subtracting the weights of two heavy objects, an evacuated sample bulb and one filled with a gas. Changes in the temperature/density of air during the course of the experiment can result in a large amount of error in your result. To prevent this, you may need to perform a buoyancy correction to your masses. When you measure the mass of your sample bulb, you will also measure the mass of a ballast bulb. The ballast bulb is a similarly sized vessel that should have a constant mass throughout the course of the experiment. If its mass changes, then we know that the room temperature/pressure has change and we need to make a buoyancy correction. The buoyancy correction is simply,
mass of Ballast Bulb (initial) – mass of the ballast bulb (final)
To correct our sample mass, we subtract the buoyancy correction from our sample mass. For example, if the mass of the ballast bulb has increased by 0.2 g, we will subtract 0.2 g from the final mass of our sample bulb.
Safety Concerns:
1. Safety goggles should be worn at all times.
2. The vacuum line is equipped with a mercury manometer. When filling the bulbs with CO2, caution must be taken not to have pressure above 1 atm.
3. When handling the sample bulb, carefully carry so that you don’t drop or break it.
4. The experiment requires the use of gases contained in cylinders equipped with a regulating valve. The cylinder must be securely strapped at all times. Consult your instructor on proper use of a gas regulator.
Procedures:
Throughout this experiment you should record the uncertainty (or notes so that you can determine ...
Experimental Determination of Compressibility Factors of Gasesiosrjce
The compressibility factor Z also known as the compression factor is the ratio of the molar volume of a
gas to the molar volume of an ideal gas at the same temperature and pressure. It is a useful thermodynamic
property accounting for real gas behavior. In general, deviation from ideal behavior becomes more significant
at lower temperatures and higher pressures. For gas mixtures, a gas composition must be specified while
calculating the compressibility factor.
Professional resume/CV for Bradley M Kremer. Mr Kremer is an international curriculum specialist and science educator based in Helsinki, Finland. He has worked in 6 countries across 3 continents.
Introduction to AI for Nonprofits with Tapp NetworkTechSoup
Dive into the world of AI! Experts Jon Hill and Tareq Monaur will guide you through AI's role in enhancing nonprofit websites and basic marketing strategies, making it easy to understand and apply.
Synthetic Fiber Construction in lab .pptxPavel ( NSTU)
Synthetic fiber production is a fascinating and complex field that blends chemistry, engineering, and environmental science. By understanding these aspects, students can gain a comprehensive view of synthetic fiber production, its impact on society and the environment, and the potential for future innovations. Synthetic fibers play a crucial role in modern society, impacting various aspects of daily life, industry, and the environment. ynthetic fibers are integral to modern life, offering a range of benefits from cost-effectiveness and versatility to innovative applications and performance characteristics. While they pose environmental challenges, ongoing research and development aim to create more sustainable and eco-friendly alternatives. Understanding the importance of synthetic fibers helps in appreciating their role in the economy, industry, and daily life, while also emphasizing the need for sustainable practices and innovation.
Read| The latest issue of The Challenger is here! We are thrilled to announce that our school paper has qualified for the NATIONAL SCHOOLS PRESS CONFERENCE (NSPC) 2024. Thank you for your unwavering support and trust. Dive into the stories that made us stand out!
Unit 8 - Information and Communication Technology (Paper I).pdfThiyagu K
This slides describes the basic concepts of ICT, basics of Email, Emerging Technology and Digital Initiatives in Education. This presentations aligns with the UGC Paper I syllabus.
June 3, 2024 Anti-Semitism Letter Sent to MIT President Kornbluth and MIT Cor...Levi Shapiro
Letter from the Congress of the United States regarding Anti-Semitism sent June 3rd to MIT President Sally Kornbluth, MIT Corp Chair, Mark Gorenberg
Dear Dr. Kornbluth and Mr. Gorenberg,
The US House of Representatives is deeply concerned by ongoing and pervasive acts of antisemitic
harassment and intimidation at the Massachusetts Institute of Technology (MIT). Failing to act decisively to ensure a safe learning environment for all students would be a grave dereliction of your responsibilities as President of MIT and Chair of the MIT Corporation.
This Congress will not stand idly by and allow an environment hostile to Jewish students to persist. The House believes that your institution is in violation of Title VI of the Civil Rights Act, and the inability or
unwillingness to rectify this violation through action requires accountability.
Postsecondary education is a unique opportunity for students to learn and have their ideas and beliefs challenged. However, universities receiving hundreds of millions of federal funds annually have denied
students that opportunity and have been hijacked to become venues for the promotion of terrorism, antisemitic harassment and intimidation, unlawful encampments, and in some cases, assaults and riots.
The House of Representatives will not countenance the use of federal funds to indoctrinate students into hateful, antisemitic, anti-American supporters of terrorism. Investigations into campus antisemitism by the Committee on Education and the Workforce and the Committee on Ways and Means have been expanded into a Congress-wide probe across all relevant jurisdictions to address this national crisis. The undersigned Committees will conduct oversight into the use of federal funds at MIT and its learning environment under authorities granted to each Committee.
• The Committee on Education and the Workforce has been investigating your institution since December 7, 2023. The Committee has broad jurisdiction over postsecondary education, including its compliance with Title VI of the Civil Rights Act, campus safety concerns over disruptions to the learning environment, and the awarding of federal student aid under the Higher Education Act.
• The Committee on Oversight and Accountability is investigating the sources of funding and other support flowing to groups espousing pro-Hamas propaganda and engaged in antisemitic harassment and intimidation of students. The Committee on Oversight and Accountability is the principal oversight committee of the US House of Representatives and has broad authority to investigate “any matter” at “any time” under House Rule X.
• The Committee on Ways and Means has been investigating several universities since November 15, 2023, when the Committee held a hearing entitled From Ivory Towers to Dark Corners: Investigating the Nexus Between Antisemitism, Tax-Exempt Universities, and Terror Financing. The Committee followed the hearing with letters to those institutions on January 10, 202
Biological screening of herbal drugs: Introduction and Need for
Phyto-Pharmacological Screening, New Strategies for evaluating
Natural Products, In vitro evaluation techniques for Antioxidants, Antimicrobial and Anticancer drugs. In vivo evaluation techniques
for Anti-inflammatory, Antiulcer, Anticancer, Wound healing, Antidiabetic, Hepatoprotective, Cardio protective, Diuretics and
Antifertility, Toxicity studies as per OECD guidelines
1. Thermal Energy and Gas Laws p. 1
MYP Year 4 Chemistry
The purpose of this investigation is to conduct a series of experiments, each of which illustrates a
different gas law. You will be given a list of equipment and materials and some general guidelines to
help you get started with each experiment. Four properties of gases will be investigated: pressure,
volume, temperature, and number of molecules. By assembling the equipment, conducting the
appropriate tests, and analyzing your data and observations, you will be able to describe the gas
laws, both qualitatively and mathematically.
OBJECTIVES
In this experiment, you will
• Conduct a set of experiments, each of which illustrates a gas law.
• Gather data to identify the gas law described by each activity.
• Complete the calculations necessary to evaluate the gas law in each activity.
• From your results, derive a single mathematical relationship that relates pressure, volume,
temperature, and number of molecules.
MATERIALS
Vernier computer interface large-volume container for water bath (at least
computer 10 cm in diameter and 25 cm high)
Vernier Gas Pressure Sensor 125 mL Erlenmeyer flask
Temperature Probe hot-water supply (up to 50°C) or hot plate
20 mL gas syringe ice
plastic tubing with two Luer-lock connectors 100 mL graduated cylinder
rubber stopper assembly with two-way valve
PRE-LAB EXERCISE
Review each of the four parts of this experiment before starting your work. You will need to decide the best
way to conduct the testing, so it is wise to make some plans before you begin. You may wish to conduct a
test run without collecting data, in order to observe how the experiment will proceed.
In each part of the experiment, you will investigate the relationship between two of the four possible
variables, the other two being constant. In this pre-lab exercise, sketch a graph that describes your
hypothesis as to the mathematical relationship between the two variables; e.g., direct relationship or
inverse relationship.
Part I Pressure, P, and volume, V (temperature and number of molecules constant).
Part II Pressure, P, and absolute temperature, T (volume and number of molecules constant).
Part III Volume, V, and absolute temperature, T (pressure and number of molecules constant).
Part IV Pressure, P, and number of molecules, n (volume and absolute temperature constant).
Advanced Chemistry with Vernier 30 - 1
2. Thermal Energy and Gas Laws p. 2
MYP Year 4 Chemistry
PROCEDURE
Part I Pressure and Volume
1. Obtain and wear goggles.
2. Position the piston of a plastic 20 mL syringe so that there will be a measured volume of air
trapped in the barrel of the syringe. Attach the syringe to the valve of the Gas Pressure Sensor, as
shown in Figure 1. A gentle half turn should connect the syringe to the sensor securely. Note:
Read the volume at the front edge of the inside black ring on the piston of the syringe, as
indicated by the arrow in Figure 1.
Figure 1
3. Connect the Gas Pressure Sensor to the Go!Link and the computer. Connect the Go!Link to the
computer using the proper cable.
4. Start the Logger Pro program on your computer. Open the file “30a Gases” from the Advanced
Chemistry with Vernier folder. This file allows you to collect pressure data from the Gas Pressure
Sensor, using Events with Entry mode. For each pressure reading you take with a button,
this mode lets you enter a volume value.
5. Measure the pressure of the air in the syringe at various volumes.
Part II Pressure and Absolute Temperature
In this experiment, you will study the relationship between the absolute temperature of a gas sample
and the pressure it exerts. Using the apparatus shown in Figure 2, you will place an Erlenmeyer flask
containing an air sample in a water bath and you will vary the temperature of the water bath.
6. Connect the Gas Pressure Sensor to 1 Go!Link and a Temperature Probe to another
Go!Link interface.
7. Assemble the apparatus shown in Figure 2. Be sure all fittings are airtight. Make sure the rubber
stopper and flask neck are dry, then twist and push hard on the rubber stopper to ensure a tight
fit.
8. Set up water baths in the large-volume container as you need them, ranging from ice water to
hot water.
9. Open the file “30b Gases” from the Advanced Chemistry with Vernier folder. This file is setup to
collect pressure and temperature data from the attached sensors, using Selected Events mode.
This mode allows you to collect a data pair simultaneously from the Gas Pressure Sensor and
Temperature Probe by clicking on the button.
Advanced Chemistry with Vernier 30 - 2
3. Thermal Energy and Gas Laws p. 3
MYP Year 4 Chemistry
Figure 2
10. Collect pressure data at several different temperatures. You must select the temperatures
yourself, but you should do it at regular intervals - either by time or by temperature.
Part III Volume and Absolute Temperature
In this experiment, you will study the relationship between the volume of a gas sample and its
absolute temperature. Using the apparatus shown in Figure 3, you will place an Erlenmeyer flask
containing an air sample in a water bath and you will vary the temperature of the water bath. Keep
some of these factors in mind as you plan your procedure.
• If you are starting with a cold-water bath, set the piston at the 0 mL mark on the syringe. This will
allow the gas volume to be increased in warmer water baths.
• The temperature of the water bath cannot be increased by more than 30-40 degrees from your
starting temperature.
• Even though you are not plotting pressure, it is important to monitor pressure in the Meter to
ensure that it remains constant.
• It is important to know the total volume of air in the flask and the syringe. The volume of the
flask, up to the bottom of rubber stopper, can be accurately measured using a graduated
cylinder. For the estimated volume of the tubing (from the rubber stopper to the Gas Pressure
Sensor box), as well as in the valve below the bottom of the syringe, use a value of ~4 mL.
11. Connect the Gas Pressure Sensor to a Go!Link and the Temperature Probe to another Go!Link
interface. Connect the interface to the computer using the proper cable.
12. Assemble the apparatus shown in Figure 3. Be sure all fittings are air-tight. Make sure the rubber
stopper and flask neck are dry, then twist and push hard on the rubber stopper to ensure a tight
fit. Be sure the water level is at least as high as the confined air in the syringe.
Figure 3
Advanced Chemistry with Vernier 30 - 3
4. Thermal Energy and Gas Laws p. 4
MYP Year 4 Chemistry
13. Open the file “30c Gases” from the Advanced Chemistry with Vernier folder. This file is set up to
collect pressure and temperature data from the attached sensors, using Events with Entry mode.
This mode allows you to collect a data pair simultaneously from the Gas Pressure Sensor and
Temperature Probe by clicking on the button and entering a value for the volume. Even
though the pressure reading will not be plotted on the graph of volume vs. temperature, it is
important for pressure to be monitored so that it can be kept constant.
14. Set up water baths in the large-volume container as you need them, ranging from ice water to
hot water.
15. Collect volume data at several different temperatures. You will select the temperatures yourself,
but make sure they are done at regular intervals.
Part IV Pressure and Number of Molecules
In this experiment, you will study the relationship between the number of molecules in a gas sample
and the pressure it exerts.
• You can use the same setup as in the previous trial, although the water bath and Temperature
Probe are optional. (Temperature must be constant, so choose a convenient temperature to run
the experiment.)
• You might be wondering how you are going to count molecules for this section. Here is a hint.
Avogadro’s hypothesis states that, “Equal volumes of gases, at the same temperature and
pressure, contain equal numbers of molecules.” Therefore, if you keep the temperature and
volume constant during the experiment, you can assume that gas volumes are proportional to
numbers of molecules. Instead of entering a total number of molecules, you could enter a total
volume of gas that has been compressed into the flask. For example, 120 mL worth of molecules
could be entered as 120 molecules, 140 mL worth of molecules would be entered as 140
molecules.)
16. Connect the Gas Pressure Sensor to the Go!Link interface.
17. Open the file “30d Gases” from the Advanced Chemistry with Vernier folder. This file allows you
to collect data from the Gas Pressure Sensor by clicking on the button and entering a
value for the number of molecules.
18. Collect pressure data with several different numbers of molecules introduced into the system.
Advanced Chemistry with Vernier 30 - 4
5. Thermal Energy and Gas Laws p. 5
MYP Year 4 Chemistry
DATA ANALYSIS - Do this part in class. The analysis should help guide the
development of your lab report.
1. For each of the four parts of the experiment, write an equation using the two variables and a
proportionality constant, k (e.g., for Part I, P = k ⋅ V if direct, or P = k/V if inverse).
2. Calculate the constant, k, for each of the four gas laws that you tested. This value can be an
average for each of the data pairs in each part of the experiment.
3. Based on the mathematical relationship and equation that you obtained in Step 1 above for each
part of the experiment, combine all four variables into a final equation. This “combined
equation” will contain P, T, V, and n, as well as a new proportionality constant, K. Be sure to
explain how you obtained your result (how you combined the equations).
4. What part of the experiments seemed to ‘work well’? Why was that the case?
5. What part(s) of the experiment did not work well? Why not? How would you change the
procedure to make your method more reliable and easier to follow? How would you change
the procedure to make the results more reliable?
6. How could you expand or change the investigation to get a ‘deeper’ understanding of the gas
laws studied in this activity?
Advanced Chemistry with Vernier 30 - 5