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Chemistry 12: Gas Laws Charles's Law
Jacques Charles
Ideal gases
Prior Knowledge/Preview
Units of temperature
Celsius and Kelvin (we won't use Fahrenheit here)
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VIDEO on Charles's Law Lab with data
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Aerospace CONNECTIONS:
Gas Laws in aerospace
Applications and examples:
Fuels--temperatures
Breathing in Space--volume/temperature in a space capsule
Temperature changes in Space
Temperature and Altitude
In the Gas Laws, we are investigating the relationships between P, V and T
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Start by studying the relationship between TWO variables at a time and keeping the third constant as well as the amount (# moles) of gas
What is kept constant?
Charles’s Law
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Investigating the relationship between volume and temperature of a gas--providing this pressure remains constant and the amount of gas (number of moles)
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Describe what's happening to the particles in the balloon
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Describe what is happening to the particles in the two balloons below
Explain WHY
Charles's Law Lab
Data collection activity:
SAFETY: Wear goggles and lab coat/apron
Care with hot objects
Method 1
Using the apparatus to the right, you will take the temperature and note the DIAMETER of the balloon for five trials at different temperatures
Do Trial #2 first when you do the actual lab--at room temperature
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Then immerse the beaker in a "freezing" solution of ice, a small amount of water and salt to get the lowest temperature in your trials.
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Measure the diameter carefully each time
Make a results table and add the data as you collect it from the trials here. If you are doing the lab you will need to add observations for your qualitative data
Use a hot plate to heat the water in the beaker--CARE with hot objects including at the end of the lab when the hotplate remains hot for some time after turning off.
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Again note the data for these higher temperature trials
Charles's Law Lab
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Analyzing data
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Looking at your data table, do you see any trends in the results obtained?
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Draw a graph--BUT in an interesting way!
Just use the top right-hand portion of the graph paper
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PLOT volume of balloon in cm^3 versus temperature in degrees Celsius
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To calculate the volume, use the formula
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BUT REMEMBER to us radius--you measured diameter. Why were you asked to measure the diameter, not the radius?
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What is the shape of the graph?
If it's a straight line there is a relationship y = mx + b
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If it goes through the origin, x is directly proportional to y: y x or y = constant times x
To get your graph to go through the "origin", extrapolate (extend) the line of the graph, so that it goes through the x axis.
Extend the scale of your graph backwards to get your experimental value of ABSOLUTE ZERO--the temperature where the gas has no volume . . .
So volume IS PROPORTIONAL to temperature--but only proportional to the absolute temperature when measured in Kelvin
Charles's Law Method 2
Here you have a thin glass tube--a melting point tube. Your teacher will prepare these with some concentrated sulfuric acid in the middle of the tube.
CARE corrosive liquid and glass--goggles and gloves and apron/lab coat
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Take the temperature of the water surrounding the tube, the height of the air trapped
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Change the temperature 5 or 6 times and note the height of the air column each time
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Draw a graph of your results--again drawing the height versus temperature in degrees Celsius on a quarter-sized sheet and extrapolating to get the value of absolute zero
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Charles's Law
Ideal gases
What are the advantages of using Method #1 with a balloon compared the Method #2 with the air trapped in a glass tube?
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What are the DISADVANTAGES of using Method #1 with a balloon compared the Method #2 with the air trapped in a glass tube?
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What method is best, in your opinion, and WHY?