KishanPatel_GasLawsDRA

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Data Reduction and Analysis [=FIERIIENT 5] Pressure, Volume, and Temperature: Discovery of the Gas Laws name: sshan Pt | parmorshame: ("2 Jahpmlle ™ Olga llovzw scten:_ 5(p (p oo (D] \]g) T scom Attached tc this page should be the following (in order): [ Tables (2) and Graphs (10, at least 2 per page). All graphs must be properly formatted. [T} Lab notebook pages. Part A: Pressure-Temperature Relationships' o ¥ inearRegresslon piot 1 | Pressure (kPa) vs. Temperature (K) Y =0.356x -1' ¥ 0.qay (, 2 | 1/Pressure (1/kPa) vs. Temperature (K) ‘fa-lmb' X+ 0.025 0,973Y4 3 | log(Pressure) (log(kPa)) vs. Temperature (K) Y=0.00r1x + 14146/ 0, Qw7 4 | Pressure (atm) vs. Temperature (K) Y =0003S%-0.2153| 0.494 ( 5 | Pressure (mmHg) vs. Temperature (K) Y = 2.069x -163.44) 0. aqH(, 6 | Pressure (kPa) vs. Temperature (°C) N =0.23506 x475.412 0.4au (y 7 | Pressure (kPa) vs. Temperature (°F) y =2.127%x 360094 0.qqy 1. Choosing between Plots #1-3, which plot shows the best relationship (i.e., most linear) between pressure and temperature? Is the relationship directly proportional, inversely pro- portional, or logarithmically proportional? Tht fPrecsure VS Tempura ture o llvin has fa best relahimnship . The ﬂlol'hov\Sh‘) is Jdivectly proportional. 2. According to the experiment, what should happen to the pressure of a gas if the temperature is doubled? Support your answer mathematically. General Equation PVanT PV=naT fo 2T P T [Pressure it double ) 27 Scanned with CamScanner

Pressure, Volume, and Temperature: Discovery of the Gas Laws 3. Which of your plots have the exact same trendline equation? Why is this the case? The Presswre va Tempoathue (1€) and The Pressuve vs. Tumpuadure (°€) hWE e exnct same frendiine equativn becawst Har presswves sty the Same, T4 S only toupahe 4. Which of your plots have the exact same R? value? Why is this the case? o g 3 Cyeits 0[01' 1 s b/fmc\ T howe e exact same rlplye becanst e only Mmat Changls with pcese plovs 1§t Uniks of tompuraduee § and 45 Conversiong, 5. Absolute zero is a theoretical temperature where matter possesses no thermal energy, i.e. the theoretical lowest possible temperature. We can roughly calculate a value for absolute zero by assuming that pressure is equal to zero. Using the trendline equations from plots 1, 6, and 7; calculate values for absolute zero corresponding to each temperature unit. General Equations: Plot A - y=0.350x - 2.9 X = ¥emp, Plot b - y= 0.35b%x +7s.4l1L Y = Pressure Plot 1- Y= 0.1a7¥x & (4,04 Pot 3 ys0.3sLx-21917 Plotl ¥=0.386x43smz LLL‘L Y201 a0 | O = 0. 42y B Y Y asux caen CC 0zo3sexr 752 R .0vH = Dula g & O 2= LSRR x= -144.161 e o x=-20.%3 x= ().2%M 6. Compare the accepted value for absolute zero to the calculated values and report percent errors. |expmmmlal value - actual uaIuel EIQ+ A i | actual value e 2-~0 o °/o Error = '&?}T—ﬂ’x 0o = 2%. 00 Plot G %o Eeror = [-20.5%3 - (-27205) | $166 =27 G54 -273.15 Plot 1 o Error = 28 -4s51.¢7 -340.206 = (-Hs4.) JrasmansiiRan) Co o0 S lom, o2 Scanned with CamScanner

Part B: Pressure-Volume Relationships b sgression Piot fendine Equatior ) {;r::;s;re (kPa) vs. Volume (mL) Y= -€. 1Y% + 204.00 |0. %14 1 |1 /Pressure (1/kPa) vs. Volume (mb) Yy = 0.000ax + 0.0007|0.4994 Elog(Pressure) (log(kPa)) vs. Volume (mL) | Y =-0.0362x + Z.HIZS o q6yY 1. Which plot shows the best relationship (i.e., most linear) between pressure and volume? Is the relationship directly proportional, inversely proportional, or logarithmically proportional? The Plot wWith LlPresswre vS Volumae wvus most lvears Tae plot was imvcm\/y {)ru»()orh‘onovl. 2. According to the experiment, what should happen to the pressure of a gas if the volume is doubled? Support your answer mathematically. General Equation PV =N D\T V=nRT 2 PV=n PA = v Presswee. -~ will reduwe by o { 147,14 5.0 4611 126. 14 g.0 1009.12 97.34 1.0 (070.1Y T8 52 14,06 (057.2% 1120 1$.0 [1DGY b2.%a ) (064.1% S4H.00 20.0 0¥ O Average [O[_{SO O"’] Standard Deviation "l 2.1702 Scanned with CamScanner

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Pressure, Volume, and Temperature: Discovery of the Gas Laws 4. Based on your data, what would you expect the pressure of your air sample to be if the volume was increased to 65 mL? Decreased to 0.65 mL? Show your work to support your answer. General Equation: pv = | 65 mL: PV =1 1L = 044,07 °’°5mL;§v~|L s i VE 65 mbl L = fut = gai— p~ lous.on p= e < {1607.§ xfA @S . < 0.65 5. For the pressure-volume study, identify the independent variable and dependent variable. What experimental variable(s) is/are kept constant? e Volume was Mme jndependomt vanable and presswed W e dependent vanable . Tempuratwre an d mo\le s weve e p ¢ Gons tan t, 6. Forthe pressure-temperature study, identify the independent variable and dependent variable. What experimental variable(s) is/are kept constant? Tempoatwre was the indqpemdent varakle and presswne was gy depmdent variable. Volume ovd mallS wWene laeld (onstant. 7. Explain the pressure-temperature relationship using the concepts of molecular velocity and molecular collisions. Pressure iy Jm,uhy reloted 4o tumpemture This waeaks « h'ﬂw,r pressure kads 1o a Wiahw 4 A wan tom re otans A hgher Keetic engy . Iinvkc 2nrgy of a molLaules s cowux\\ic Jujm‘ wfic'- <lastic Han.s.on > U wn [X4% wWoWu waLen boAweshn © molcwules , [Kiathe guergy of o w9 tat the Jveloes oF A wolcauk 8. Youperformed the experiment using air, which we know is actually a mixture of several gases. w i}l iacreAs£s Would the results of this experiment be improved if we used a sample of pure nitrogen? Why or why not? The results of WS experiment would be improved \As'-v\S A Sampe of pure nikpgen bt camse ush\fi | e dype of gas can Create i+ un S’\Vc Calculation s 30 poteat £xror, Precise vasults thot |owe Less Scanned with CamScanner

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