Absolute Kelvin Temperature of the Absorbed Atmosphere was Duplicated: Voltage Doubles Also - Assignment Example

Running head: Gas Laws (Boyles and Charles Laws) Student’s name Institution Course Professor Date of Experiment Date of Submission Abstract This report describes the experimental analyses that were used to determine the relationship between pressure and volume and also between pressure and temperature. In both experiments, sealed cylindrical tubes were used. In part one of these experiments, an open-tube manometer was used to attest Boyle’s Law. The temperature of the trapped gas was assumed to be constant during experiment. In part two of the experiment, a quantity of air was trapped between the sealed end of cylindrical tube and a movable plug of mercury where the temperature could be changed. The volume of the trapped air was kept constant. . Pressure of the air at different temperatures was measured with a view to find out the relationship between the pressure of the air and its temperatures at constant volume. Graphs of pressure against volume and pressure against temperature were plotted and compared with the empirical data. The Y-intercept, b was determined, the slope, m was calculated and the temperature at zero was calculated using the equation y=m x + b. These results and errors were analyzed and discussed. TABLE OF CONTENTS Abstract 2 TABLE OF CONTENTS 3 1.0Introduction 4 1.1Theory 4 2.0 Methodology 7 3.0 Procedures 7 3.1 Experiment A (Part I) 7 3.1.1Calculation and Results 7 3.1.2 Discussion 10 3.2 Experiment B (Part II) 10 3.2.1 Calculation and Results 10 3.2.2Discussion 13 4.0Conclusion. 13 5.0 Experimental Errors 14 6.0 References 15 1.0Introduction This report describes the experimental analyses that are utilized to determine the relationship between pressure and volume and between pressure and temperature. These relationships are demonstrated by Boyle’s Law, Gay-Lussac’s law and Charles’ law. In part one is to determine how the volume of a gas will change with pressure for a constant amount of gas and temperature and also to determine how the pressure of a gas will change with the temperature for a fixed amount of gas and volume. In the second experiment, a quantity of air will be trapped between the sealed end of cylindrical tube and a movable plug of mercury (Myers, 2006). Pressure of the air at different temperatures was measured with a view to find out the relationship between the pressure of the air and its temperatures at constant volume (Loyd, 2008). Theoretically, in an ideal gas, there is a direct relationship between volume and temperature and pressure and volume. Both the particulate nature of matter and the kinetic theory of gas influence the study of properties of ideal gases. The aims of the experiments were: 1) To familiarize with the equipment used in the experiment 2) To verify Boyle’s Law 3) To verify Charles’s Law and Gay-Lussac’s law and determines the absolute zero temperature. 1.1Theory Boyle’s law, Charles’ law and Gay-Lussac’s law give the relationships between pressure, volume and temperature for an ideal gas. They are used to predict how gases can behave when they are subjected to different conditions. Boyle utilized a J-shaped piece of glass tubing that was sealed on one end. The air in the sealed end of the tube was to adjust the pressure of the system (Myers, 2006). Pressure can be adjusted and the volume of the gas can be determined. Boyle’s law assesses the relationship between pressure and volume with constant amount of gas and temperature. Thus the law states that for a fixed amount of gas at constant temperature, the pressure of the gas varies inversely with the volume (Pople, 1987).It can be mathematically expressed as PV=K Where P= pressure V= the volume K= a constant Charles’s law illustrates the relationship between volume and temperature. For instance, Where V= volume occupied by an ideal gas T=Temperature of the gas in kelvins K= a proportionality constant dependent on the number of moles and the pressure of the gas Gay-Lussac’s Law states that the pressure and Kelvin temperature of a gas are directly proportional at a constant volume (Loyd, 2008). P= Pressure of trapped air T=Temperature of the gas in kelvins Absolute zero can be termed as the temperature at which the volume drops to zero. It is used to envisage how a change in pressure will alter the volume of the gas and vice versa (Loyd, 2008). For instance, increasing the temperature of a confined gas will increase the kinetic energy of the gas molecules and can results in more collisions of the molecules with the walls of the containers. The value of absolute zero can be arrived at by measuring the pressure of a gas sealed in a constant-volume container at different temperatures and extrapolating to a pressure of 0 atm (Pople,1987).The volume and temperature are much related, for example, if the temperature is not efficient, the molecules will not be able to overcome the weak forces of attraction or fill the container (Loyd, 2008). At 0 K, there is no kinetic energy (absolute zero) and volume. Pressure Law states that: for a given amount of a gas at a constant temperature, the pressure of the gas is indirectly related to the volume. In order to attest this law, a graph of inverse of gas volume versus gas pressure is needed (Myers, 2006) Temperature has been known as a measure of the relative movements of particles in a substance since it is a measure of the average kinetic energy of the particles. Those particles with huge kinetic energy have a tendency to collide frequently and move apart (Pople, 1987). Thus, the forces that bind some molecules together at a particular temperature are greater than the kinetic energy of the molecules (Goodwin, 1990). 2.0 Methodology Materials and equipment employed during the two experiments were Sealed cylindrical tube that could be adjusted 3.0 Procedures 3.1 Experiment A (Part I) First, one was required to familiarize with the sealed cylindrical tube. The release valve was open to set the pressure to atmospheric, O on the gauge (1 BAR absolute). The connecting rod was pulled out to the 50ml volume position, as seen when the first (red) calibration mark on the connecting rod was viewed. The release valve was then closed and the connecting rod was pulled out till the second calibration, 100ml was brought into view and the meter reading was then recorded. The process was carried on until the 150ml, 200ml and 250ml marks were reached. At each volume both pressure and temperature were recorded. The experiment was repeated five times. From the results, the average value of pressure for each volume was calculated. With the help of values of p, the actual pressure in pounds per square inch and also in Pascals at each volume was calculated. Lastly, the results were compared with Boyle’s Law and a graph was drawn. N/B- This experiment was carried out quickly due to incidence of leakages during the process. 3.1.1Calculation and Results In part I, the results were as tabulated as follows 1 2 3 4 5 Average pressure 100ml 0.8 0.7 0.7 0.8 0.75 0.75 150ml 0.6 0.6 0.65 0.66 0.6 0.622 200ml 0.4 0.45 0.45 0.4 0.4 0.42 250ml 0.3 0.3 0.35 0.3 0.3 0.31 The average value of pressure, p for each volume and the actual pressure in pounds per square inch and in Pascals are shown in the table below Volume of gas (ml) Volume of gas (1/V) Average pressure (BAR) Absolute value of Pressure (Bar) Actual pressure in Pounds per square inch (psi) Actual pressure in Pascals (Pa) 100ml 0.01 0.75 1.75 25.35psi 175000pa 150ml 0.0067 0.622 1.622 23.525psi 162200pa 200ml 0.005 0.42 1.42 20.595psi 142000pa 250ml 0.004 0.31 1.31 18.999psi 131000pa 3.1.2 Discussion From the graph, the slope (gradient) can be calculated by 7.89/ (-190.8) -0.04135 The slope is a straight line and negative and it illustrates that as the volume of the ideal gas increases the pressure decreases. Thus it validates the Boyle’s law that there is an inverse relationship between pressure and volume of a given amount of gas at constant temperature. 3.2 Experiment B (Part II) A sealed cylindrical tube was utilized in this experiment within which the temperature of the gas could be changed. In this experiment, the silicon tube was disconnected from the nozzle on the end of the apparatus in order to reset the pressure in the apparatus to ambient. Then the silicon tube was reconnected again from the nozzle on the end of the apparatus. The values of both temperature and pressure were recorded. The heating element was turned on and the temperature and pressure readings every 10 seconds were recorded. A graph of temperature against pressure was plotted. The gradient was compared with the constant volume law. 3.2.1 Calculation and Results In Part II, the results were tabulated as follows Pressure Temperature in Celsius Temperature in Kelvins 52.3 24 297 53 24 297 53.5 24 297 54 24 297 54.8 26 299 55.5 26 299 56 27 300 57 28 301 57.7 29 302 58.5 29 302 60 30 303 63 31 304 64.5 32 305 65 35 308 65.7 37 310 66.1 37 310 67 37 310 3.2.2Discussion From the graph, the slope (gradient) can be calculated by 1.79 Y=m x + c Y intercept is 27.99 atm and the absolute zero temperature is -25 °C The percentage error 9.16% Furthermore, the graph depicted that when the absolute Kelvin temperature of the trapped air was doubled, its pressure doubles also and also dividing the pressure of the air by its absolute temperature (Kelvin) gave the same value. Thus the pressure of a fixed mass of gas is directly related to its absolute temperature so long as the volume of the trapped air is kept constant (Pressure law). 4.0Conclusion. In the above experiments, the relationship between pressure and volume in a fixed gas sample was determined. Also, the relationship between pressure and temperature in a fixed volume of gas was determined. A sealed cylindrical tube was used in both experiments. From the graph, the pressure of the gas is inversely proportional to the volume at a fixed temperature. A graph of pressure against temperature was used to estimate the value of the absolute zero temperature. The pressure increases uniformly as the temperature increases. 5.0 Experimental Errors Possible source of errors was the set-up of the cylindrical tube that may have some leakages. 6.0 References David H. Loyd,”Physics Laboratory Manual, Volume 10”: Cengage Learning, 2008.Print Myers, R. L, “The Basics of Physics”, Westport, CT: Greenwood Publishing Group, 2006. Print. Peter Goodwin, “Practical Physics Labs: A Resource Manual”, Walch Publishing, 1990.Print Pople, S, “Explaining Physics Gcse”, (Ed 2) Oxford: Oxford University Press, 1987. Print. Robert Bruce Thompson, “Illustrated Guide to Home chemistry Experiments: All Lab,” O’Reilly Media, Inc., 2002 T. L. Lowe, John F. Rounce,”Calculations for A-level Physics”, Nelson Thornes, 2002 Read More