Gas Laws Experiment - Coursework Example

Gas Laws Experiment General Introduction The gas laws were developed in eighteenth century when scientist realized that there was some relationship that was there between the volume, pressure and the temperature of given sample of gas. This relationship was postulated to be true to all gases irrespective of its physical features. Normally have a similar behavior to the colossal extent of conditions because all gases tend to have their molecules that are widely spaced. The equation that is obeyed by gases is called the equation of state that is derived from the kinetic theory of gases. There are various gas laws, but all are considered to be some particular forms of the ideal gas equation which contains some constant (s). There are different gas laws that exist and are summarized by the equation of state (Meyer, 2011). These gas laws include Boyle’s law, Charles law, Gay – Lussac’s law and other gas law. Part 1: Boyle’s Law Purpose Experiment to investigate the correlation between pressure and volume of a gas. Background The Boyle’s law was derived, finalized and published in 1662. The law states that when gas is at constant temperature, the product obtained from the volume, and the pressure of a certain mass of gas that is confined in a closed system is always a constant. The pressure gauge can be used to verify this statement together with a variable container capacity. The law can also be derived from the kinetic theory of ideal gases. For instance, if a gas container has a fixed number of molecules in it and its volume is reduced more molecules will collide per unit time per given area. This aspect results in a higher pressure in the container (Wang, 2013). The mathematical expression of the law is as shown below: …. (1) PV = k1 or P1V1 = P2V2 …… (2) Where, P – The pressure of the gas. V – The volume of the gas. K1 – The constant of the equation. Procedure 1. Reset the pump and give it a firm push. Wait until the value stabilizes. Observe whether the values of the pump after stabilizing the same? 2. Select the light species of the box on the right-hand corner. You can notice that the pump turns red. At that time, the pump is given a press. Again, wait for the values to stabilize and observe the results. 3. In the box entitled box control move the arrow and remove it and find what happens. The height of the gas container should be 5.3 nm, and the depth is 230 nm. Data Table 1: values of gas pressure and volume at constant temperature. 100 heavy particles constant temperature 300 k° length volume pressure nm nm^3 atm Pascal 9.00 10971.0 0.40 40530.00 8.50 10361.5 0.42 42556.50 8.00 9752.0 0.45 45596.25 7.50 9142.5 0.49 49649.25 7.00 8533.0 0.51 51675.75 6.50 7923.5 0.55 55728.75 6.00 7314.0 0.60 60795.00 5.50 6704.5 0.65 65861.25 Analysis Graph 1: pressure against volume at constant temperature Discussion When the pump is pressed it some while to come to the stable state. When the pump gives a substantial push the volume of the gas reduced. For this experiment volume in an independent variable, since it does depend on the other parameter to change. The pressure is the dependent variable as it depends on the volume change for it to vary. The graph was plotted for the values of the pressure, and the volume showed that the pressure of the gas varies inversely proportionally to the volume of the gas. Conclusion The relationship between the pressure and the volume of gas under constant temperature is summarized by the Boyles Law. This law states the under constant conditions of temperature, gas will have its pressure vary inversely proportional to the volume. Part 2a: Experiment on Charles’ Law Purpose Determination of the relationship between temperature and volume at constant pressure. Background Charles’ Law is also referred to as the law of volumes. It was founded in 1787 by a scientist by the name Jacques Charles. It states that the amount of given mass of gas at constant conditions of pressure is directly proportional to the absolute temperature when in a closed system. The mathematical expression of the law is as shown below (Kotz, Treichel and Townsend, 2010). V T ……… (2) V/T = k2 … (3) It can be summarized as V1/T1 = V2/T2 …… (4) In the above T is the Kelvin temperature of the gas, while V is the resulting volume of the gas at given temperature. Procedure N.B.: To hold pressure constant, the container will be filled some percentage with some gas in it before the start of the experiment. This step is done to ensure that the atmospheric pressure inside the container is not equal to zero. 1. Heat the container while measuring the corresponding values of the volume while keeping the pressure constant (don’t add any gas molecules to the container). 2. Record the readings for various values of the volumes corresponding to the temperature. Data Table 2: Values of volume and temperature of a gas at constant pressure. 100 heavy particles constant pressure (0.22 atm) temperature length Volume Kelvin° nm nm^3 450 9.2 11214.8 400 7.9 9630.1 350 6.3 7679.7 300 5.9 7192.1 250 4.8 5851.2 200 4.5 5485.5 150 3.5 4266.5 100 2.2 2681.8 Analysis The data was plotted in a graph of volume against temperature. The following figure was obtained. Graph 2: Graph of volume against temperature. Discussion In this experiment, the temperature component is an independent variable, and the volume is the dependent variable where it depends on the temperature. In this experiment, there are 2 factors that are held constant, which are pressure and the number of the molecules of the gas. The graph obtained of the volume against temperature is a straight line that does not pass through the origin. Conclusion The relationship of the volume and the temperature of a gas at constant number of molecules and constant pressure are illustrated by the Charles’ law. The law holds for all gases that obey the equation of state. Part 2b: Gay- Lussac’s Law Experiment Purpose Determination of the relationship between the temperature and the pressure with other conditions held constant Background Gay- Lussac’s law is also referred to as the Pressure law and was founded by Joseph Lussac in 1809. The law states that for an ideal of perfect gas the pressure that will be exerted on the sides of the container will be directly proportional to the Kelvin temperature. This aspect occurs at constant volume and a given mass of gas (Crosland, 2002). The mathematical expression of the law is as illustrated below. P T …………… (5) P/T = k3 ……… (6) P1/T1 = P2/T2 ….. (7) Where P- the pressure of the gas. T – The absolute temperature of the gas. Procedure 1. Put some gas content in the container and connect it to the pressure gauge. 2. Heat and cool the container and observe the pressure change on the gauge. 3. Note about eight values of the temperatures and the corresponding pressures. 4. Tabulate the data in a table and plot a graph of the pressure against temperature. Data Table 3: values of pressures and temperature at constant 100 heavy particles constant volume 8533nm^3 temperature pressure Kelvin° atm Pascal 300 0.48 48636 315 0.52 52689 330 0.54 54715.5 345 0.57 57755.25 360 0.59 59781.75 375 0.62 62821.5 390 0.65 65861.25 405 0.67 67887.75 Analysis The above data was plotted on a graph of pressure against temperature. Graph 3: A graph of pressure against temperature. Discussion The graph obtained was a straight line graph showing that the pressure varies directly proportionally with absolute temperature. Conclusion The relationship illustrated above summarizes the law that connects the pressure and the temperature of a gas at constant volume and constant moles of gas. Part 3: Relationship between particles and pressure Purposes Determining the relationship particles and pressure when other conditions are held constant (Kardar, 2008). Procedure The temperature of the particles is held constant, and volume is also held constant. 1. Using a non-elastic container put some molecules of gas and measures the corresponding value of the pressure. 2. Continue adding more gas particles while measuring the values of the pressure. 3. Tabulate the data obtained. Data Table 4: values of pressure and amount of particles constant temperature 350k constant volume 5635 nm^3 number of pleasure particles atm pascals 100 0.59 59782 125 0.74 74981 150 0.83 84100 175 0.99 100312 200 1.18 119564 225 1.27 128683 250 1.4 141855 275 1.52 154014 Analysis The data was utilized to plot a graph of pressure against number of particles. Graph 4: a graph of pressure against number of particles Discussion All other conditions were kept constant except the pressure and the number of particles. The number of particles was the independent variables. The pressure is a dependent variable that depends on the number of particles. There were factors of volume and temperature that were held constant during the experiment. Conclusion The relationship of pressure exerted on the wall of the container in directly proportional to the number of particles, when other conditions are held constant. References Crosland, M. (2002). Gay-Lussac. Cambridge: Cambridge University Press. Kardar, M. (2008). Statistical physics of particles. New York, NY: Cambridge University Press. Kotz, J., Treichel, P. and Townsend, J. (2010). Chemistry & Chemical Reactivity. Australia: Brooks/Cole. Meyer, S. (2011). Gases and their Properties. New York: Rosen Pub.s/ Rosen Central. Wang, S. (2013). Gas laws. [S.l.]: University-Press Org. Read More