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# Temperature Experiment

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Change is influenced by many different factors in many different situations. If you imagine the 400,000 gallons of water in a stream at the top of a hill, you can picture that they will flow down the hill in order to reach equilibrium. But what if the temperature outside is -40 degrees Fahrenheit? How might this change the movement of the water molecules down the hill?
This is a virtual lab. The demonstration uses red and blue balls to represent molecules. . Items that should be recorded for submission are written in italics.
1. Go to http://chemconnections.org/Java/molecules/index.html
3. For both the Red side and the Blue side, move the slider labeled "Mass" all the way to the right (the value should read 199 amu). You should see the balls in the window above get larger.
Each of these balls represents a molecule moving around inside a divided chamber. You can see how the molecules move around randomly until they bump into a wall or into each other.
4. Lower the temperature on the Red side of the chamber by moving the slider labeled "Temperature" all the way to the left (the value should read 1 K).
*Compare the movement of the molecules on the very cold Red side with the molecules on the Blue side. How does lowering their temperature change the speed at which these molecules move?
5. Now lower the temperature on the Blue side of the chamber to 1 K, the same way you did in Step 4.
6. Add lots more molecules to both sides by increasing the slider labeled "Number" all the way to the right (the value should read 99) for both the Red and the Blue side.

*How would adding more molecules affect the motion inside the chambers?
7. Click the "Remove Barrier" button and time how long it takes for the blue and the red molecules to mix completely (note: the button text may not appear on your screen. The "Remove Barrier" button is on the far lower right).

*Record this result as "Mixing at 1K"
8. Click the "Reset" button (note: the button text may not appear on your screen. The "Reset" button is just to the left of the "Remove Barrier" button). Then, repeat steps 3-6 above. Once you have 99 slow-moving molecules in each chamber, increase the temperature in both chambers to 999 K. You should see two very active chambers!

9. Click the "Remove Barrier" button on the lower right and time how long it takes for the blue and red molecules to mix completely.

*Record this result as "Mixing at 999K"
10. *In a paragraph, describe your results and explain the effect temperature appears to have on the equilibrium of mixing.

11. *Based on your virtual lab experiment, compare what would happen if you put a spoonful of honey into a cup of 200 degree Fahrenheit tea versus placing a spoonful of honey into an identical cup filled with 45 degree Fahrenheit tea.

12. *If you opened up a container of very stinky Limburger cheese at one end of an empty large outdoor parking lot with a group of shoppers about 50 feet away. Would you be able to enjoy eating your snack longer without offending the shoppers in the summer or the winter? Explain.

https://brainmass.com/chemistry/experimental-design-and-methods-in-chemistry/temperature-experiment-267888

#### Solution Summary

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## Experiment to demonstrate the Ideal Gas Law.

Experiment to demonstrate the Ideal Gas Law.
Attached is the directions and data sheet. Here is the link for the data sheet. http://www.mhhe.com/physsci/physical/giambattista/thermo/thermodynamics.html

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Data and related questions
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Part 1

P (Pa) V (m^3) T(K)
498.6 5 300
453.27 5.5 300
415.5 6 300
383.53 6.5 300
356.14 7 300
332.4 7.5 300
311.62 8 300
293.29 8.5 300277 9 300
262.42 9.5 300
249.3 10 300

P (Pa) V (m^3) T (K)
249.3 10 300
262.42 9.5 300
277 9 300
293.29 8.5 300
311.62 8 300
332.4 7.5 300
356.14 7 300
383.53 6.5 300
415.5 6 300
453.27 5.5 300
498.6 5 300
554 4.5 300
623.25 4 300
712.28 3.5 300
831 3 300
997.2 2.5 300
1246.5 2 300
1662 1.5 300
2493 1 300

When we held the temperature constant and cut the volume in half, each time we reduced the volume we observed that the pressure (increased/decreased) by a factor of (1 / 2 / 4 /8 / 10). Circle the correct answer.

When we held the temperature constant and reduced the volume from 10 to 1, we observed that the pressure (increased/decreased) by a factor of ( 1 / 2 / 4 / 8 / 10). Circle the correct answer.
Part II

P (Pa) V (cm^3) T (K)
831 1 100
831 2 200
831 4 400
831 8 800
831 10 1000

When we held the pressure constant and double the temperature, each time we doubled the temperature we observed that the volume (increased/decreased) by a factor of ( 1 / 2 / 4 / 8 / 10). Circle the correct answer.

When we held the pressure constant and increased the temperature from 100 to 1000, we observed that the volume (increased/decreased) by a factor of (1 / 2 / 4 / 8 / 10). Circle the correct answer.

Part III

P (Pa) V (cm^3) T (K)
166.2 5 100
332.4 5 200
664.8 5 400
1329.6 5 800
1662 5 1000

When we held the volume constant and doubled the temperature, each time we doubled the temperature we observed that the pressure (increased/decreased) by a factor of (1 / 2 / 4 / 8 / 10). Circle the correct answer.

When we held the volume constant and increased the temperature from 100 to 1000, we observed that the pressure (increased/decreased) by a factor of (1 / 2 / 4 / 8 / 10). Circle the correct answer.

Part IV

(a.) We observed that as we compress the gas (decrease the volume) the temperature (increased/decreased) and pressure (increased/decreased). Circle the correct answers.

(b.) We observed that as we compress the gas (decrease the volume) the molecules moved (faster/slower) Circle the correct answer.

(c.) As we compressed the gas the temperature (increased/decreased) and kinetic energy of the molecules (increased/decreased) and the molecular activity (increased/decreased). Circle the correct answers.

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