Absolute Zero Lab

The End

Conclusion

In this lab, we found that our hypothesis was correct because we hypothesized that the volume of the gas would rise linearly with the temperature of the water. From our data, we can conclude that this is true because our data points aligned together, causing them to be directly proportional. Not including our outlier, our data almost lined up with the predicted results to reach absolute zero. Using the slope of our results, we calculated the volume of the gas to be -5.690 mL at absolute zero.

Evaluation

Absolute Zero Lab

Our two sources of error were:

• Not providing ample amounts of time to reach equilibrium.
• Not exact because some heat was lost in the transfer and measuring of the plunger.

Analysis

Our two modifications were:

• Giving more time for the gas and water to reach equilibrium.
• Have better equipment to get even more precise results.

The relationship between IV and DV: The relationship between the volume of gas and the temperature of the water was that they were directly proportional.

By: Chris Loo

Andreas Bello

Josh Long

Andrew Norman

Outlier: Our point 6 was furthest from our best fit line. This was because we did not let the plunger settle long enough to get accurate results.

Prediction Question: What would the volume of the gas be at 475.5K?

Temp. of water X Slope + Y-intercept = Volume

Graph

Slope = 0.05009 mL/K

Data

Procedure

Materials

Water temp (°K) = Water temp (°C) + 273

· Syringe w/ cap

· 4 Beakers (700 ML each)

· 4200 mL of Tap Water

· 3 Thermal Containers (each holds 1000 mL and one is labeled for salt water trials)

· Tongs

· Lab Quest (with temperature probe attachment)

· Hot Plate

· Ice

· Salt

· Small Amount of Gas

1. Fill a beaker with 700 mL of water

2. Place the temperature probe in the water, wait for the water to reach thermal equilibrium with the room. Then pour the water into a thermal container.

3. Move the plunger to the 10 ml mark.

4. Place the temperature probe in the water. Then place the syringe (using tongs) in the water. The entire syringe, minus the plunger must be submerged in water.

5. Wait for the temperature probe to stop changing temperature (reach thermal equilibrium).

6. Once it reaches equilibrium, take the probe out. Measure the volume of gas in the plunger. (Push the plunger in and let the syringe settle by itself for the most accurate results).

7. Pour out the water.

8. Repeat step 1

9. Heat the beaker on low, until it reaches 326 degrees Kelvin . Once at 326 degrees, pour the water into a thermal container.

10. Repeat steps 3-7.

11. Repeat step 1

12. Heat the beaker on medium, until it reaches 343.7 degrees Kelvin. Then pour into a thermal container.

13. Repeat steps 3-7.

14. Repeat step 1

15. Heat the beaker on high, until it reaches 372.5 degrees Kelvin. Pour into thermal container

16. Repeat steps 3-7.

17. Repeat step 1

18. Put the beaker in ice until it reaches 280.2 degrees Kelvin. Pour the water into a thermal container.

19. Repeat steps 3-7.

20. Repeat step 1

21. Apply salt to the water and stir until dissolved. Put the beaker in ice until it reaches 271.2 degrees Kelvin. Pour the water into the thermal container.

22. Repeat steps 3-7.

Hypothesis

If the temperature of water changes, then the volume of the gas will mimic the change in water linearly because they are directly proportional.

IV, DV, Constants

IV: The initial temperature of the water

DV: The volume of the gas in syringe

Constants: Source of water, Thermal containers, Beakers, Temperature probes, Syringe (and cap), Tongs

Testable Question

What is the relationship between temperature of water and volume of gas?