LAB 1 phy

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William Rainey Harper College *

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132

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Apr 3, 2024

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UIC Physics Department Physics 132 Laboratory Report Boyle’s Law Page 8 of 9 NAME Barkha Patel LAB SECTION (Day & Time) Wednesday 5-6:50pm DATE 01/23/2023 Physics 132 – Lab # __ 1 __ Title Boyle’s Law Pre – laboratory Assignment Carefully read the description of the lab 1. Describe in your own words the overall goals of the lab. To estimate the Gas Constant R. To also understand the Boyle’s law. Determine the relationship between pressure and volume at constant temperature of an ideal gas ( air ) and compare the experimental results with theoretical prediction. 2. Identify the physics concepts that you will learn about or test in the lab. Boyle's law states that at constant temperature the volume of a given mass of a dry gas is inversely proportional to its pressure. We will also use the ideal gas law PV=nRT, to find the gas constant. P is inversely proportional to V. 3. Describe briefly what you will measure in the lab and make your prediction of the most important outcomes of the experiment. We will measure pressure using a machine, volume of the syringe. In a syringe, the volume of a fixed amount of gas is increased by drawing the plunger back, thereby lessening the pressure. Jongho Lee _________________________________________________________________ _________________________________________________________________________________________________________________________

UIC Physics Department Physics 132 Laboratory Report Boyle’s Law Page 1 of 9 Boyle’s Law (Experimental Procedure and Data Analysis) This part of the lab must be completed entirely independently of your lab partner(s) or other students. Make sure that you avoid unauthorized collaboration and plagiarism. All suspected violations of the Standards of Conduct will be referred to Student Judicial Affairs. Lab Section (Day & Time): _ Wednesday at 5-6.50pm_________ Name: ____ Barkha Patel ______________________________________ Station #: ______ 1. Make sure that the power for the Pasco Interface 850 is turned on. 2. Check that the Pressure Sensor is plugged into the Pasport Sensor 1 port on the interface and the 60 mL syringe is connected via silicone tubing to the pressure sensor and two-way valve as shown in Figure 1. 3. Open Pasco Capstone software from the desktop. 4. Click Hardware Setup under Tools on the left and check that the pressure sensor is recognized by the interface . 5. Drag “Digits” dispay into the center of the workspace. On the display, click <Select Measurement> and choose “Absolute Pressure (kPa)”. The computer screen should look something like Figure 2. 6. Turn the two-way valve to the open position. The diagram below shows what this looks like. 7. To measure atmospheric pressure click “Record” button in “Control” menu. The atmospheric pressure value measured by the sensor will appear on display. Figure 2 Figure 1

UIC Physics Department Physics 132 Laboratory Report Boyle’s Law Page 2 of 9 8. Record the atmospheric pressure measured by sensor and the room temperature below. 𝑃 ௔௧௠,௦௘௡௦௢௥ = _____ 99.51 ______ kPa 𝑇 ௥௢௢௠ = ____ 23 ___  C Then click “Stop” button to terminate recording. The acceptable range of values is 101.6  3.3 kPa . If it does, then the apparatus is ready for use. If it does not, contact immediately your Lab TA or Lab Assistant. 9. Record the atmospheric pressure, 𝑃 ௔௧௠,௖௠ு௚ (in centimeters of Mercury, cmHg), shown by a room barometer. 𝑃 ௔௧௠,௖௠ு௚ = _____ 75.6 ____ cmHg Convert the atmospheric pressure in centimeters of mercury to kilopascals (1 cmHg = 1.33 kPa) and record its value below. 𝑃 ௔௧௠,௕௔௥௢௠௘௧௘௥ = _____ 100.55 ________ kPa Question 1. Are the atmosperic pressures measured by sensor and barometer the same. If not, why do they differ from each other? They are the same because there is range in which they belong. The sensor, syringe and two-way valve are attached to each other by silicone tubes and we need to estimate the volume of air trapped in the tubes. There are two kind of silicone tubes used, 0.32 cm and 0.64 cm in diameter. Use a ruler to estimate the volume of air trapped in the tube attached to the syringe by using the following equation 𝑉 ௧௨௕௘ = 𝜋 ቀ ௗ ଶ ቁ ଶ 𝐿, where d is diameter and L is the length of the tube, and record its value below. (53.2cm=L, d=0.32cm) 𝑉 ௧௨௕௘ = ________________ cm 3 Now, let’s look at the relationship between volume and pressure

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UIC Physics Department Physics 132 Laboratory Report Boyle’s Law Page 3 of 9 10. Set the syringe plunger to the 40 cm 3 and turn the two-way valve to the closed position. The diagram to the right shows what this looks like. Note: Measure the volume at the position of black rubber seal marked with red arrows as shown in the figure to the right, not at the inverted V-shaped projection. The syringe barrel has major scale divisions marked every 5 milliliters (1mL = 1 cm 3 ), and minor scale divisions every 1.0 mL. The volume should be estimated to within ±0.5 mL. 11. click “Record” button and slowly push the plunger in to 38 cm 3 position. 12. When you reach the the plunger final position, record the pressure, P , in Table 1 and then click “Stop” and open two-way valve and set the syringe plunger back to the 40 cm 3 mark. 13. Calculate the total volume 𝑉 = 𝑉 ௦௬௥௜௡௚௘ + 𝑉 ௧௨௕௘ and record the result in Table 2. Repeat steps 10 – 13 for the final syringe volumes listed in Table 1 (three times for each volume). 14. Estimate the uncertainties in volume measurements, 𝜎 ௏ and record the values in Table 2. Explain your reasoning. _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _________________________________________________________________________________________________________________________ 15. Calculate 1/𝑉 and the uncertainties in these values, 𝜎 ଵ/௏ , and record the results in Table 2. 16. Calculate the average pressure, 〈𝑃〉, for each volume and record the results in Table 2. 17. Make a reasonable estimate of uncertainty in pressure measurements, 𝜎 〈𝑷〉 , and record its values in Table 2. _________________________________________________________________________________________________________________________ _________________________________________________________________________________________________________________________ _________________________________________________________________________________________________________________________ 𝑉 ௦௬௥௜௡௚௘ (cm 3 ) Trial #1 Trial #2 Trial #3 𝑃 (kPa) 𝑃 (kPa) 𝑃 (kPa) 40 38 36 34 32 30 Table 1

UIC Physics Department Physics 132 Laboratory Report Boyle’s Law Page 4 of 9 _________________________________________________________________________________________________________________________ _________________________________________________________________________________________________________________________ _________________________________________________________________________________________________________________________ 18. For each volume, V , calculate PV and record its values in Table 2. 19. Calculate the average value , 〈𝑃𝑉〉 and its uncertainty, and write its value below 〈𝑃𝑉〉 = ______________________  _________________ kPa  cm 3 20. Calculate the uncertainties associated with PV , 𝜎 ௉௏ , and record the results in Table 2. 21. Use the graph paper on page 7 (labeled with “ P vs 1/V graph”) to plot a graph of pressure on the y-axis versus 1/V on the x-axis. Add error bars on the graph and draw a best-fit line through the data. Note: The origin of the graph should be (0,0). Choose a suitable scale for each axis so that the data points fill the graph as completely as possible. 𝑉 (cm 3 ) 𝜎 ௏ (cm 3 ) 1/𝑉 (cm  3 ) 𝜎 ଵ/௏ (cm  3 ) 〈𝑃〉 (kPa) 𝜎 〈௉〉 (kPa) 𝑃𝑉 (kPa  cm 3 ) 𝜎 ௉௏ (kPa  cm 3 ) 0.233 3989 0.1888 3958 0.8639 3904 0.3003 3828 0.7792 3752 0.16978 3682 Table 2

UIC Physics Department Physics 132 Laboratory Report Boyle’s Law Page 5 of 9 23. Use the graph paper on page 7 (labeled with “ PV vs V graph”) to plot a graph of the PV on the y-axis versus V on the x-axis. Add error bars on the graph. Add a line representing the 〈𝑃𝑉〉 value. P vs 1/V graph

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UIC Physics Department Physics 132 Laboratory Report Boyle’s Law Page 6 of 9 Question 2. Do the error bares overlap the line representing the 〈𝑃𝑉〉 value? Yes/No _________________ Question 3. Is there evidence for a systematic error in any of your measurements of pressure and/or volume? State clearly your evidence either for or against the presence of a systematic error. Yes , because across all 3 trials we had slightly different values for P when looking at specified volumes. 25. Use your results and Eq. (3) to estimate the Gas Constant, R . Note: Dry air has density 1.2 kg/m 3 and its molar mass is 28.97 g/mol. _________________________________________________________________________________________________________________________ _________________________________________________________________________________________________________________________ _________________________________________________________________________________________________________________________ _________________________________________________________________________________________________________________________ _________________________________________________________________________________________________________________________ _________________________________________________________________________________________________________________________ ________________________________________________________ PV vs V graph y = 0.0309x - 83.951 R² = 0.9833 0 5 10 15 20 25 30 35 40 45 3600 3650 3700 3750 3800 3850 3900 3950 4000 4050 4100 PV (kpa.cm 3 ) Volume (cm 3 ) PV vs V

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