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Lab 8: Using the Ideal Gas Law Lecture & InstructionsPage
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Lab 8 Using the Ideal Gas Law
CHEM101L
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Access Code (located on the lid of your lab kit): Click here to enter text.
Lab Report Format Expectations
Utilize college level grammar and professional formatting when completing this worksheet.
Report all equations in a proper mathematical format, with the correct signs and symbols.
Pre-Lab Questions”
1. This lab includes two experiments, one in which you will experimentally determine the
relationship between volume and temperature, and another in which you will observe the rate
of gas evolution from a catalytically driven reaction. What types of measurements will you take
in this lab in order to study these phenomena?
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2. Atmospheric pressure varies with the altitude (or height above sea level) of your location. How
would you expect the air pressure to change if you went from sea level to Denver, Colorado,
which is 1.5 kilometers (1 mile) above sea level? Why would you expect the pressure to be
different?
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3. In Experiment 2, you will use a catalyst to drive a chemical reaction. What are catalysts and why
are they used in chemical reactions?
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Lab 8 Using the Ideal Gas Law
CHEM101L
EXPERIMENT 1: CHARLES’ LAW
Introduction Questions
1. What is the overall purpose of Experiment 1? What results do you expect and why?
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2. What does Charles’ Law state regarding the relationship between pressure, volume and
temperature. Explain each of these three variables as they pertain to this law.
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3. In this experiment, you will assume that you can draw a straight line through the Temperature
and Volume data you observe. Why can you do this?
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Lab 8 Using the Ideal Gas Law
CHEM101L
Data and Observations
Record your temperature and volume measurements in the table below.
Table 1: Temperature vs. Volume of Gas Data
Temperature Conditions
Temperature (˚C)
Volume (mL)
Room Temperature
Input
Input
Hot Water
Input
Input
Ice Water
Input
Input
Insert a photo of your experimental setup, ensuring that you show the correct lab items used.
Lab 8 Using the Ideal Gas Law
CHEM101L
Below, you will insert a graph of your Temperature and Volume data. To earn credit for this lab, follow
the instructions below to generate a precise graph that will allow you to answer the questions in the
Results and Discussions section. It is highly suggested to use graph paper or graphing software. Ensure
that your name is included. A graph that does not satisfy the requirements below will not be accepted.
Steps to graph:
1. Draw an X axis from -300C to 100C.
2. Draw a Y axis that starts at 0°C and extends upward to the maximum of your volume
measurements. For example, if your highest volume was 5 mL, ensure your Y axis extends just
past 5 mL.
3. Plot your volume, temperature data. You should have 3 points total.
4. Use a ruler, or graphing software, to draw a line through the points. Do not simply connect the
dots. (The line might not touch any of your points. That is okay as this is only a line of best fit.)
5. Ensure that your line slopes upward from left to right.
6. Extend the line that goes through your points to the X axis.
7. Include a copy or photo of your graph below, ensuring your name is included.
Lab 8 Using the Ideal Gas Law
CHEM101L
Results and Discussion
1. What happened to the volume of gas when the syringe was exposed to various temperature
conditions? Using the concepts explored in the Introduction, describe why this occurred,
keeping in mind the definition of temperature.
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2. What does the line that you drew through your data represent?
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3. Why can you assume a linear relationship? Said in other words, why can you draw a straight line
through the data?
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4. At what temperature does your line intersect the x-axis? What volume corresponds to this
temperature?
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5. What does that temperature represent? Do you think it would be possible to cool the gas in the
syringe down to that temperature? Why or why not?
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EXPERIMENT 2: USING THE IDEAL GAS LAW
Introduction Questions
1. What is the purpose of this experiment? What is it attempting to demonstrate?
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2. The ideal gas law equation is PV=nRT. Explain each of the variables in this equation.
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3. This experiment will involve the decomposition of hydrogen peroxide into water and oxygen.
Write a balanced chemical equation for this process.
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Lab 8 Using the Ideal Gas Law
CHEM101L
4. You will need to show the ambient pressure of the room in which you are conducting this
experiment. Provide the source you will utilize for this pressure reading, along with a general
location of where it corresponds to (city, state, region are all acceptable).
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Data and Observations
In the tables below, record your temperature and volume measurements.
Table 2: Temperature, Pressure and Volume Data
Temperature
of Distilled
H O:
Initial Volume
of Air (mL)
Final Volume of Air
(after reaction) (mL)
2
Ambient
Pressure
(atm):
Volume of O Collected
(Final Volume – Initial
Volume)
Input
Input
Input
Input
Input
2
Table 3: Reaction Time Data
Time Reaction
Started
Input
Time Reaction Ended
Total Reaction Time
Input
Input
Below, include a photo of your experimental setup showing the reaction as it is taking place. To earn
credit for this lab, you must clearly depict the correct lab setup and clearly depict the reaction taking
place. Include your handwritten name in the photo.
Lab 8 Using the Ideal Gas Law
CHEM101L
Results and Discussion
1. Based on your observations, gas was evolved and collected in the graduated cylinder. Where did
that gas come from?
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2. What would happen if you added more than five mL of yeast to the H2O2?
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3. What would happen if you added more than 5 mL H2O2 to the 5 mL of yeast?
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4. How would the number of moles (n) of O2 change if your atmosphere was doubled and all other
variables stayed the same?
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Lab 8 Using the Ideal Gas Law
CHEM101L
5. Using the Ideal Gas Law (PV = nRT) calculate the grams of O2 produced in the reaction (Hint:
solve for n, and then convert moles to grams. Don’t forget to convert your temperature from
Celsius to Kel-vin.) You must show all your work for credit
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