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Determining the relationship between the pressure and volume of a confined gas - Boyle's Law

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Introduction

´╗┐cambridge high school Investigating Boyle?s Law Studying the relationship between the pressure and volume of a confined gas Thaer Al-Kilani Session #: Candidate Name: Thaer Al-Kilani Supervisor Name: Ban Darwish Grade: 11 IB ________________ 1. Design ________________ ________________ 1. Research Question ________________ How does different volumes (20, 25, 30, 35, 40, 45, 50, 55, 60) ml of a confined gas (air) affect its pressure? ________________ ________________ 1. Hypothesis ________________ As the volume of a confined gas is decreased, the gas particles will exert more pressure inside the syringe as the particles will collide more frequently with each other and with the syringe. According to Boyle?s law, the relationship between the volume of a confined gas and the pressure it exerts is inversely proportional, for as the volume is halved, the pressure is doubled at a constant temperature. ________________ ________________ 1. Variables ________________ ________________ 1. Independent Variable ________________ The independent variable is the Volume of the confined gas (Air) which ranges between 20 ml and 60 ml (20, 25, 30, 35, 40, 45, 50, 55, 60) ...read more.

Middle

121.6 121.6 121.6 121.6 0.040 136.5 137.4 136.5 136.8 0.035 155.1 155.1 155.1 155.1 0.030 179.4 179.4 179.4 179.4 0.025 212.0 217.6 212.9 214.2 0.020 265.1 263.3 261.4 263.3 1Volume of Confined Gas (Air) 2Pressure of Confined Gas (Air) 3Average Pressure of Confined Gas (Air) 1. Data Processing ________________ 1Volume(dm30.0005) 1/Volume (dm-3) Mass of trapped gas (g) Number of Moles (moles) 3Average Pressure Tav 0.060 16.67 0.074 0.0025 91.8 0.055 18.18 99.9 0.050 20.00 109.8 0.045 22.22 121.6 0.040 25.00 136.8 0.035 28.57 155.1 0.030 33.33 179.4 0.025 40.00 214.2 0.020 50.00 263.3 Table 2.2 shows processed data after being recorded from the experiment * Mass of trapped gas Example: 1Volume(dm30.0005) Mass of trapped gas (g) 0.060 0.074 * Mass of trapped gas = g ________________ *D = 0.001225 g/cm3 ________________ *Volume of trapped gas (Air) in cm3 ________________ ________________ jghs.edin.sch.uk. <http://www.jghs.edin.sch.uk/departments/mathscience/chemistrynotes/highernotes/chemistryhighernotes/moles_and_energy.pdf>. ________________ * Number of Moles Example: 1Volume(dm30.0005) Mass of trapped gas (g) Number of Moles (moles) 0.060 0.074 0.0025 * Number of Moles = moles ________________ *Molar Mass of Air = 28.96 g/mole ________________ *Mass of trapped gas (Air) ________________ Utc.edu. ...read more.

Conclusion

The hypothesis deduced can be justified by stating that when the volume of a gas in a confined manner is decreased, the gas particles collide with each other and with the walls of its surrounding more frequently as there is less space, hence they exert more pressure. Overall, the results of this experiment prove Robert Boyle?s Mathematical relationship regarding the Volume and Pressure of a confined gas which is: PV = nRT 1. Evaluation ________________ In such an experiment, random errors which would increase the rate of error would include changes in the temperature of the surrounding (causing changes in the temperature of the syringe), presence of impurities or any other different gas other than air in the syringe.Such random errors might have decreased the precision of this experiment. On the other hand, Systematic errorstransfer of heat from the hand of the pupil onto the syringe when handling it (causing fluctuations in the temperature), movement of the piston away from the desired mark at high pressures (causing changes in pressure), or leakage of air through the syringe or the data logger (causing changes in pressure). Such systematic errors will result in limited or decreased accuracy of the experiment. ________________ ________________ Page | ...read more.

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