Katie Hodder Gas laws lab report

pdf

School

Memorial University of Newfoundland *

*We aren’t endorsed by this school

Course

1010

Subject

Chemistry

Date

Feb 20, 2024

Type

pdf

Pages

Uploaded by ConstableSharkPerson1046

Katie Hodder November 23rd, 2023 Chemistry lab report “Gas Laws” Results: Table #1 “Pressure and Volumetric data table” Pressure (kPa) Volume (mL) 88.36 kPa 15.7 mL 109.30 kPa 12.7 mL 130.00 kPa 10.7 mL 79.89 kPa 17.7 mL 66.83 kPa 20.7 mL *added 0.7 to each volume recorded for less error*

Table #2 “Pressure and Absolute Temperature” Pressure (kPa) Temperature (C) 108.97 kPa 50.80 C 104.71 kPa 36.50 C 101.70 kPa 24.10 C 98.25 kPa 18.30 C 96.92 kPa 10.10 C

Table #3 “Determination of the Gas Law Constant, R” The mass of Magnesium solid used 0.0133 g Amount of Hydrochloric acid used 10 mL **Moles of H ₂ gas 0.00055 mol The volume of gas in the eudiometer tube 13.9 mL = 0.014 L Temperature of water 22.7 C Temperature of gas 295.85 K Barometric pressure (P atm) 765 mm Hg Vapour pressure of water 20.70 mm Hg **Pressure of H ₂ gas (P H ₂ ) 765 mm Hg 1.007 atm R-value 0.086 J / mol·K Sample Calculations: Mols of H ₂ gas: 0.0133g x 1 mol/24.31g = 0.0005471 mols → 0.00055 mol H ₂ R-value: (1.0066 b) (0.0139 L) / (0.0005471 mol) (295.85 K) = 0.08646 J/mol·K Pressure of H ₂ gas (P H ₂ ): P H ₂ = nRT/V P H ₂ = (765 mm Hg)(0.086 J/ mol·K)(295.85 K) / 0.014 L P H ₂ = 1.007 atm % error R-value: R actual - R calculated / R actual x 100% = 0.0821 - 0.086 / 0.0821 x 100% = 4.75%

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

Discussion: Concerning Volume versus pressure, when the volume of water increases, the pressure decreases. Boyle's law states that the volume of a given mass of gas varies inversely with the pressure when the temperature is kept constant. An inverse relationship is described in this way. As one variable increases in value, the other variable decreases 1 . When volume is decreased, the molecules present begin striking the walls of the container they are contained in; this increases the pressure. When volume is increased, the molecules have a greater distance between them and the wall, and they will hit the walls of the container less often, causing a decrease in pressure. When comparing the pressure and temperature of gases, as the temperature increases, the pressure follows and increases as well. Gay-Lussac’s law states that the pressure of a gas is directly proportional to the absolute temperature, provided the volume and amount of gas are not changed. 2 When a gas is heated, the molecules gain more energy and move faster. The more times the molecules hit the wall of the container, the more pressure there is; therefore, as temperature increases, so does pressure. The percent error for my R-value is 4.75%. The reasons for errors in this lab could vary. One of the possible errors I noticed was the presence of bubbles on the copper wire after the magnesium solid dissolved. This could add to the error percentage because the volume recorded from this experiment was not completely accurate, as the presence of air bubbles tampered with the volume. The possibility of gas leakage from an improperly sealed container is another possible source of error. As a result, the experiment's gas volume will fluctuate over time, affecting the readings and producing discrepancies between the experiment's results and theoretical values. With the temperature and pressure experiment, possible errors that may change the results could be human error; due to the fact that laboratories are not perfect, human error occurs constantly. As a result, errors of this kind could always occur, including perception errors, equipment problems, and measurement errors. When it comes to the third part of this lab; the calculations of R-value possible errors may be created from the beginning of the experiment. When reading the volume level on the eudiometer tube, if the volume is read wrong the R-value will be less accurate. 2 “7.4: The Pressure-Temperature Relationship.” Chemistry LibreTexts , Libretexts, 3 Apr. 2023, chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introduction_to_General_Chemistry_(Malik)/ 07%3A_Gases/7.04%3A_The_pressure-temperature_relationship#:~:text=Gay%2DLussac’s%20law %20states%20that,1%3DP2T2. 1 “14.3: Boyle’s Law.” Chemistry LibreTexts , Libretexts, 8 Aug. 2022, chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/14%3A_Th e_Behavior_of_Gases/14.03%3A_Boyle’s_Law#:~:text=Boyle’s%20law%20states%20that%20the,val ue%2C%20the%20other%20variable%20decreases.

The Ideal Gas Law states that under the same temperature, pressure and volume all gases contain the same number of molecules (but not the same mass) 3 .Real gases exhibit behavior that differs significantly from ideal gases, especially at high pressures. The behavior of real gases only approaches ideal gas behavior at relatively low pressures. At higher temperatures, the behavior of real gases also resembles that of ideal gases. Because gas molecules have very little space between them, real gases behave very differently from ideal gases at high pressures and low temperatures. This ois why the data I collected shows the when temperature increases pressure also increases, but when volume increases pressure decreases. This is because the gas in this lab was a real gas rather than an ideal gas. The ratio of \(PV/nRT\) is less at low temperatures than it would be for an ideal gas; at low temperatures, this impact is especially noticeable for complex and simple gases. The effect of nonzero molecular volume prevails at very high pressures. The minimum shown in the PV/nRT versus P plot for many gases is caused by a conflict between these effects. Conclusion: In this experiment the volume and temperature changes in gas were compared to the pressure changes in gas. This experiment showed that as temperature increases, pressure also increases, and as volume increases, pressure decreases. This lab also challenges teamwork skills, measuring skills, and math skills. The results from this lab proved that we worked with abreal gas rather than an ideal gas and the lab proved the importance of attention to detail as the smallest mistake could create errors become present in the data results. 3 “The Ideal Gas Law (PV = NRT) (Video).” Khan Academy , Khan Academy, www.khanacademy.org/science/ap-chemistry-beta/x2eef969c74e0d802:intermolecular-forces-and-pro perties/x2eef969c74e0d802:ideal-gas-law/v/ideal-gas-equation-pv-nrt#:~:text=So%2C%20in%20sum mary%2C%20the%20Ideal,into%20a%20liquid%20or%20solid. Accessed 25 Nov. 2023.

Related Documents

1_Sci_Investigation_worksheet_F21.docx

CHM110 Pre-Lab 4.docx

Macrotheme 1 f2023oc.pdf

gen chem II LG iv - exam 1 review (key).pdf

General Chemistry 1 Lab Manual_Student_10_24_22.pdf

Experiment 2. Sodium Borohydride Reduction_Experimental Procedure - REVISED W24.pdf

Solubility+Curve+Lab+v2.pdf

Recommended textbooks for you

Introductory Chemistry: A Foundation

Chemistry

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:Cengage Learning

Introduction to General, Organic and Biochemistry

Chemistry

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:Cengage Learning

Chemistry

ISBN:9781305957404

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

Publisher:Cengage Learning

SEE MORE TEXTBOOKS

Recommended textbooks for you

Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning