Good Sample Lab Report (1)

docx

School

Philadelphia University *

*We aren’t endorsed by this school

Course

101

Subject

Chemistry

Date

Jul 2, 2024

Type

docx

Pages

Uploaded by CommodoreExploration4001

Confirm Gas Laws . Prof. Cebula .

Introduction Gas molecules move at random and collide with each other unexpectedly. The distance between the molecules is largely dependent on the temperature the substance is at. Pressure, temperature, and volume are all related to gas expansion. Most gases function in the same way. The ideal gas law formula works for any gas at a lower density or a high temperature. Experimental Details For this experiment, I used the PhET “Gas Properties” lab from Colorado University Boulder. To begin the experiment, I had to confirm Boyle’s Law, PV= K I added 50 “light” molecules and changed the volume of the box while keeping the temperature constant. As the volume decreased, the pressure increased. As the volume increased, the pressure decreased. Initial (trial 1) Initial (trial 2) Final (trial 1) Final (trial 2) Pressure 2.4 atm 2.2 atm 6.2 atm 1.6 atm Volume (width) 15.0 nm 7.9 nm 5.0 nm 13.4 nm Boyle’s Law: PV= K Trial 1- Initial: (2.4 atm)(15.0 nm)= 36 Final: (6.2 atm)(5.0 nm)= 31 Trial 2- Initial: (2.2 atm)(7.9 nm)= 17.38 Final: (1.6 atm)(13.4 nm)= 21.44 This confirms Boyle’s law because the constants are very close. These numbers will not be exact because it is an experiment. Image 1. This image shows the end result of Boyle’s Law.

The next part of the experiment was to confirm Charles’ Law, V/T= K Once again, I added 50 “light” molecules and changed the volume of the box while keeping the pressure constant. As the temperature increased, the volume increased and vice versa. Initial (trial 1) Initial (trial 2) Final (trial 1) Final (trial 2) Temperature 58 K 124 K 95 K 178 K Volume (width) 8.6 nm 9.7 nm 14.0 nm 13.9 nm Charles’ Law: V/T= K Trial 1- Initial: (8.6nm)/(58K)= .15 Final: (14.0nm)(95K)= .15 Trial 2- Initial: (9.7nm)/ (124 K)= .08 Final: (13.9 nm)/ (178 K)= .08 This confirms Charles’ law because the constants are the same. Image 2. This picture shows the end result of Charles’ Law. The last part of this experiment was to confirm Gay-Lussac’s Law, PT= K I added 50 “light” molecules again and changed the temperature while keeping the volume constant. As the temperature was increased, the pressure also increased. Initial (trial 1) Initial (trial 2) Final (trial 1) Final (trial 2) Temperature 163 K 60 K 199 K 42 K Pressure 3.2 atm 1.4 atm 2.6 atm 2.0 atm Gay-Lussac’s Law: P/T= K Trial 1- Initial: (3.2 atm)/(166 K)= .0193 Final: (5.7 atm)/(294 K)= .0194

Your preview ends here

Eager to read complete document? Join bartleby learn and gain access to the full version

Access to all documents
Unlimited textbook solutions
24/7 expert homework help

Trial 2- Initial: (1.4 atm)/(62 K)= .023 Final: (0.9 atm)/(40 K)= .023 This confirms Gay-Lussac’s law because the constants are very similar. They will not be exact because the pressure is constantly changing. Image 3. This Image shows the end result of Gay-Lussac’s Law. Results Each of these results yield the same constant from initial to final experiments. In Boyle’s and Gay- Lussac’s Laws, the constants are not exactly the same. This is because the pressure is always changing and never constant. Each of the calculations below are theoretical values. Theoretical Values and % Errors of each trial 1: Boyle’s Law Initial: (2.4 atm)(15.0 nm)= 36 Final: (6.2 atm)(x nm)= 36 X= 5.8 nm % Error= (5.0-5.8)/5.8 *100=13.8% error Charles’ Law Initial: (8.6nm)/(58K)= .15 Final: (14.0nm)/(x K)= .15 X= 95 K % Error= (95-95)/95 *100= 0% Error Gay-Lussac’s Law Initial: (3.2 atm)/(166 K)= .0193

Final: (5.7 atm)( x K)= .0193 X= 295 K % Error= (294-295)/295 *100= .33% Error Each of these values allows us to see how mathematically each component is related. In Boyle’s Law, as pressure increases, volume decreases. In Charles’ Law, as volume increases, temperature increases. In Gay-Lussac’s Law, as pressure increases, temperature increases. These values correspond to the experimental values because the components do the same thing in terms of increasing and decreasing. Each percent error shows how accurate the values in the experiment were. The Boyle’s Law confirmation experiment had a 13.8% error. This is because the pressure was constantly changing so I just had to pick a value within the range. The Charles’ Law confirmation part had a 0% error because the pressure was held constant, and I could accurately read the values. The Gay-Lussac’s Law had a .33% error which is almost perfect but once again this is because the pressure reading was always changing. Discussion Each of these values, both experimental and theoretical, confirm how each law corresponds with its volume, pressure, and temperature. Each law consists of each component, and one holds constant. In Boyle’s law, temperature is constant, in Charles’ law, pressure is constant, and in Gay-Lussac’s law, volume is constant. The percentage errors for each part of the experiment also allowed me to see how each of the experimental values were off because of the constant pressure changing. Conclusion and Summary Overall, this lab allowed me to see how pressure, temperature, and volume interact with each other. These three laws being confirmed help show the relationship between the components. When volume is constant, pressure and temperature are inversely related, when pressure is constant, volume and temperature are directly related, and when temperature is constant, pressure and volume are inversely related. I believe that I now have a much better understanding of how all the components of gases are related. References 2.1 molecular model of an ideal gas - university physics volume 2 . OpenStax. (n.d.). https://openstax.org/books/university-physics-volume-2/pages/2-1-molecular-model-of-an- ideal-gas Gas Properties - Phet Interactive Simulations. (n.d.). https://phet.colorado.edu/sims/html/gas- properties/latest/gas-properties_en.html

Related Documents

Unit 19 Blood Lab Report-1.pdf

Screenshot 2024-06-29 211642.png

Dosage calculation quiz.docx

Lab 5 Heat (1).pdf

Lab 1- CHM2045L Tiffany F PDF.pdf

CHEM 110 Exp08 Data Sheet.docx

lab 9.docx

MATH 302_Week 5Test_Q3_Q4 Attempt1.docx

Organic Farming Essay.pdf

Integrated Rate Law practices.pdf

Isolation of Caffeine from a Tea Bag.edited (2).docx

Q7.png

Recommended textbooks for you

Chemistry

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Cengage Learning

Chemistry

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Cengage Learning

Chemistry: Matter and Change

Chemistry

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Glencoe/McGraw-Hill School Pub Co

Chemistry: The Molecular Science

Chemistry

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:Cengage Learning

SEE MORE TEXTBOOKS

Recommended textbooks for you

Chemistry
Chemistry
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning