How the Ideal Gas Law Applies to Real Physical Experiments
Student: Wanda Mattson Rhodes Date: March 12, 2015 Partner: Tiara Key Introduction Section: 721 The objective of this lab was to examine how the Ideal Gas Law applies to real physical experiments. Using the Ideal Gas Law, we were able to find absolute zero and the universal gas constant. An ideal gas is a gas that is composed of a set of randomly moving non-interacting point particles. The Ideal Gas Law is given by the equation: iv = nor Where p = pressure (Pa) V = volume (mm) n – number of moles (mol) R = Universal Gas Constant T = temperature (K). Couture Collect Beakers of different Ethanol and Ethylene Glycol mixtures with ratios of 00, 25:75, 50:50, 75:25, 100:0 percentages of mixture. Place dry ice in each beaker.
For each mixture ratio use lab quest to determine the temperature and pressure of each mixture. Record all data and plot graph. Rest Its The results of our experiment Showed that percentages with a higher Ethylene glycol content had a higher pressure, but lower temperature compared to the mixtures with higher Ethanol content.In our lab we noticed accurate trends in pressure and temperature. We also observed that Ethanol had a lower pressure at 1 00%, than Ethylene Glycol at 100% As shown in the graphs below Discussion In out lab experiment for the most part we measured everything accurately when it came to recording temperature and pressure of the Ethanol and the Ethylene Glycol mixtures. The one thing that I did notice a trend in is the longer the dry ice sat in the mixtures compared to when it was first submerged the pressure and temperature changed relatively.So I think in this experiment our calculations are off because we were measuring the pressure and temperature of the mixtures all at different times after the dry ice had been submerged into the mixtures.
Conclusion In conclusion this lab indeed did show us trends of pressure and temperature that we should have seen. While pressure increases, temperature decreases, and when Pressure decreases temperature increases.