Paraphrased essay

Sara Muttaleb Section 04423 April 2020 Deriving gas laws using computer simulation Data Table 1: Pressure vs Volume ( with constant temperature at 300 k ).Trial Pressure Val (atm)Width (nm) Depth (nm) Height (nm) Volume ( )nm31 11.3 15.0 04.0 8.75 5252 12.5 14.0 04.0 8.75 4903 13.5 13.0 04.0 8.75 4554 14.5 12.0 04.0 8.75 4205 15.7 11.0 04.0 8.75 3856 17.5 10.0 04.0 8.75 3507 19.4 09.0 04.0 8.75 3158 22.2 08.0 04.0 8.75 2809 24.5 07.0 04.0 8.75 24510 29.5 06.0 04.0 8.75 21011 35.2 05.0 04.0 8.75 175 Observation: The gas particles condense move around quicker and at a shorter distance. As length decreases, pressure increases at a higher rate.Table 2: Temperature vs volume with constant pressure at 17.5 atm.Trial Temperature (K)Width (nm) Depth (nm) Height (nm) Volume ( nm3)Initial : 300 10.0 04.0 8.75 5251 373 12.0 04.0 8.75 4902 282 09.0 04.0 8.75 4553 262 08.8 04.0 8.75 4204 243 08.1 04.0 8.75 3855 226 07.7 04.0 8.75 3506 205 07.0 04.0 8.75 3157 190 06.6 04.0 8.75 2808 177 05.8 04.0 8.75 2459 157 05.5 04.0 8.75 21010 135 05.0 04.0 8.75 175 Observation: As temperature increases, volume decreases. Table 3: Temperature vs pressure with volume held constant at 10.0 nmTrial Temperatur e (k)Pressure (atm)Width (nm) Depth (nm) Height (nm)Volume ( )nm31 104 5.5 10.0 04.0 8.75 3502 204 11.5 10.0 04.0 8.75 3503 305 18.1 10.0 04.0 8.75 3504 407 23.3 10.0 04.0 8.75 3505 508 29.9 10.0 04.0 8.75 3506 610 35.5 10.0 04.0 8.75 3507 706 41.4 10.0 04.0 8.75 3508 801 47.3 10.0 04.0 8.75 3509 904 52.2 10.0 04.0 8.75 35010 1014 59.5 10.0 04.0 8.75 350 Observation: As we increase the temperature, the pressure increases as well. Table 4: Pressure vs quantity and temperature held constant at 300 K.Trial Pressure (atm)Quantity of gas particlesTemperat ure (K)Width (nm)Depth (nm)Height (nm)Volume ( )nm31 17.7 150 300 10.0 04.0 8.75 3502 29 250 300 10.0 04.0 8.75 3503 40.4 350 300 10.0 04.0 8.75 3504 52.5 450 300 10.0 04.0 8.75 3505 64.5 550 300 10.0 04.0 8.75 3506 77.7 650 300 10.0 04.0 8.75 3507 87.7 750 300 10.0 04.0 8.75 3508 99.1 850 300 10.0 04.0 8.75 3509 110.1 950 300 10.0 04.0 8.75 35010 115.7 1000 300 10.0 04.0 8.75 350Observation: As pressure is increasing we notice a significant increase in the quantity of gas particles.Analysis Procedure: Pressure Volume Relationship 1.Fig.1 Graph representing the relationship between volume and pressure at constant temperature. 2.Fig 2 Graph representing the relationship between inverse volume and pressure at a constant temperature. 3.​ The relationship between volume and pressure is an inverse relationship because as pressure increases, volume decreases when the temperature is held constant. The ideal gas equation is PV=nRT, where pressure and volume are equated to n, moles, r, Boltzmann constant, and t, temperature. Boyle’s law equation PV=K, where pressure and volume are equated to constant temperature.4. ​We were asked to graph the inverse volume to state Boyle’s law that pressure is inversely proportional to a constant temperature P=1/V. Analysis Procedure 2: Volume Temperature Relationship 5.Fig 3. Graph representing the relationship between temperature and volume with constant pressure at 17.5 atm. 6. ​The relationship between volume and temperature is directly proportional. As volume increases, temperature increases. In the equation . for the initial volumeV 1 T 1 = V 2 T 2 V 1 T 1 and temperature of the gas and stand for the final volume and temperature.V 2 T 2 7. ​The temperature is in Kelvin units at the y-axis, it represents the temperature of the gas that we are measuring the volume of. ​ ​Y= 0.568x+33.1. The slope of the graph is 0.568.Analysis procedure 3: Temperature Pressure Relationship 8.Fig 4. Graph representing the relationship between pressure and temperature at a constant volume 9. ​When the volume is held constant PV=nRT can be rearranged to . ThisP 1 T 1 = P 2 T 2 relationship is directly proportional as the pressure goes up, the temperature also goes up and vice-versa. Increasing the temperature causes the gas particles to move faster. When we hold the volume of the gas constant , the pressure and temperature will increase. 10. ​Temperature is heat. Heat causes molecular motion to increase causing more speed between the particles. So when temperature decreases, volume and pressure would decrease too. As temperature decreases, the pressure decreases too which causes the molecular motion of the gas particles in the tank to slow down. This will cause the volume to shrink due to the slow movement. 11. ​ Pressure of the gas is due to molecular motion with the walls, so if the motion stops at absolute zero, I would expect the pressure and the volume of a gas sample will also become zero. The pressure is 0 atm at absolute zero and all the molecular motion stops.Analysis Procedure 4: Pressure Quantity Relationship 12.Fig 5. This graph represents the relationship between quantity of particles and pressure. 13. ​The more increase in the number of gas particles in the container, the higher the pressure. Adding zero particles will cause the pressure to be at zero and it slowly increases as we add particles to the tank. I would say yes, this should be the same for all gases. 14.​ When the number of moles increases, the volume and pressure increases as well. In the equation v/n=k express if temperature and pressure remain constant. Therefore, the volume of gas has a proportional relationship with the number of moles of gas. If the number of moles increase, the volume of gas increases. 15.​ The slope of the pressure vs quantity of particles relationship graph is 0.116. The full equation is y=0.116x+0.385. If the temperature is constant, then the value should be the same to other gases as well. Citation: Tro, Nivaldo J. (2017). Chemistry; A Molecular Approach. Pearson Education.
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