Law What Valid for Practical Gases at Comparatively Low Pressures - Assignment Example

GAS LAWS NAME: STUDENT NO: COURSE: MODULE: DATE OF EXPERIMENT: DATE OF SUBMISSION: Abstract For proper understanding in areas of physics, it is ideal to study the gaseous physical behavior. This behavior in gases is governed by the empirical gas laws, which are the Charles’s and Boyle’s gas laws. The explanation of the empirical gas laws is dated in 18th century describing the behavior of the gases in gearing towards the industrial revolution in the development of the steam engine. In the 19th century, thermodynamic implications on the application of the empirical gas laws remain as implied by the kinetic behavior of the gases. This kinetic behavior of the gases remains valid up to today to explain the thermodynamic of the empirical gas laws. This experiment investigates the behavior of the gases using some of the empirical gas laws, which will help in determining the universal gas constant. Experiment I, relates volume and pressure and thus it investigates the existence and validity of Boyles law, which is an empirical gas law. Further, experiment II is a relation between pressure and temperature, thus it investigates the validity and existence of the ideal gas law. Introduction Ideal gas law relates the pressure and temperature of gas as directly proportional. Thus, combined gas law indicates that volume of a given gas charges with change in temperature in the vessel that contains the gas that has determined number of moles and at constant pressure. Where: p =pressure, V= volume of the gas, R = universal gas constant, T= is temperature Thus for a fixed volume, and R is constant then, Where: P pressure of the gas and T is the temperature causing change in volume at that instant. Thus, for given different temperatures it leads to different pressure for given gas. This is given in the relation:  Evidently, this is the ideal gas law, which relates pressure and temperature of a given gas. However, the law is only valid for real gases at relatively low pressures and high temperatures (Darrell & Steven1860. Thus, the law does not apply at absolute zero temperature. On the other hand, Boyle’s law relates volume and pressure of a given gas as inversely proportional given as: Where; P = pressure V = gas volume and  is constant value for the pressure volume relation. Therefore, this experiment is an investigation of the two empirical gas laws, the Boyle’s and Charles gas laws. Experimental objectives The key objective of this experiment is to investigate the empirical gas laws and determine the behavior of the gases at varying conditions. Materials and methods Part I The materials needed for part included: Cylindrical tube Gas release valves Meter Methods 1. I had to familiarize with the equipment. 2. I had to set the gauge pressure to 0 by opening the release valve, and pulled the connecting rod to the 50 ml mark as indicated by the red (first) calibration mark. 3. Next I closed the release valve and pulled out the connecting rod to the next 100 ml mark and recorded the meter reading, while perfoming the experiment quickly because there were leakages. 4. I repeated (3) above for 150ml, 200ml and 250ml, recording the pressure and temperature at each volume. 5. I did 5 times steps 1to 4 for each volume recording pressure at each 6.  The data recorded is given below: Table 1: volume and pressure Volume (ml)  (bar)  (bar)  (bar)  (bar)  (bar) Average P 100 0.8 0.7 0.7 0.8 0.75 0.75 150 0.6 0.6 0.65 0.66 0.6 0.622 200 0.4 0.45 0.45 0.4 0.4 0.42 250 0.3 0.3 0.35 0.3 0.3 0.31 Part II Materials needed: Water manometer Silicon tube Cylindrical tube Heating element Thermometer Methods and procedure used 1. First I had to familiarize with the equipped to use 2. To reset the pressure in the apparatus to ambient I disconnected the silicon tube from the nozzle on the end of the apparatus 3. I recorded the initial temperature and pressure of the experiment 4. I turned on the heating element and recorded the temperature and pressure difference readings at a span of 10 second as indicated in table 2 Table 2: pressure and temperature Pressure Temperature 52.3 24 53 24 53.5 24 54 24 54.8 26 55.5 26 56 27 57 28 57.7 29 58.5 29 60 30 63 31 64.5 32 65 35 65.7 37 66.1 37 67 37 Results and discussion Part I of the experiment is an investigation on the application and effect of change in volume to pressure of a given gas. Evidently, the experiment is ideal and is a clear indication that the gas obeys the Boyle’s law since it follows that volume is inversely proportional to pressure exerted by the gas. In addition, from table 1, pressure of the gas reduces as the volume increases and thus this meets the aim of the experiment, to investigate the effect of volume on pressure of a given gas (Steven 45). The pressure-volume relation is a plot of the average pressure measured with increase in volume of the gas and clearly indicates that pressure and volume graph obeys the Boyle’s law, which is an explanation of the experimental results. Part II of the experiment investigates pressure temperature relationship, which is the explanation for ideal gas law. As the aim of the experiment is to obtain results relating to prove gas laws, it is clear from the results obtained from the experiment; the pressure-temperature relation follows the ideal gas law. The ideal gas law is valid only for the ideal gases and thus at absolute zero temperature, that is, at -273k, the law is not applicable for the gas (Richard 109). Therefore, this means the experiment was conducted at ideal standard room temperature and pressure. Therefore, from the graph of pressure-temperature, the curve will meet the x-axis at -297K, which is not ideal for real gases since gases liquefy before they reach that temperature. Thus, it gives a discrepancy of the temperature difference. Conclusion From the experiment, there exists the absolute pressure and gas molecule relation. Since it is possible to increase the pressure by simply adjusting the volume and temperature of the gas, when the gas particles in a given gas doubles they result to double the pressure. Thus, gas pressure is directly proportional to the number of molecules in the gas. Thus for the gas laws, there must be a relation between different factors which range from pressure, temperature and volume. Therefore, for a low density gas pressure is proportional to the temperature and changes with inverse proportion to the volume. This equation is summarized in ideal gas law with R, which is the universal gas constant. Moreover, the gas constant gives the gas an ideal gas behavior. Works Cited Richard, Myers. The basics of chemistry. New York: Greenwood Group, 2003. Darrell, Ebbing & Steven, Gammon. General Chemistry. New York: Cengage Learning, 2010. Steven, Zumdahl. Chemical Principles. New York: Cengage Learning, 2009. Read More