chemistry 1 lab

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please find the attachment and follow the instructions to fill it thanks. please find the attachment and follow the instructions to fill it thanks. please find the attachment and follow the instructions to fill it thanks. please find the attachment and follow the instructions to fill it thanks.

NAME:_______________________ DATE:_______________________ LAB INSTRUCTOR:_______________________ Lab Exercise 11 - Simulation Behavior of Gases: Finding the Molar Mass of a Fictitious Gas Using Temperature and Average Velocity OBJECTIVES • Determine the molar mass of a fictitious gas in a simulation • Learn the relationship between temperature and kinetic energy INTRODUCTION The molecules of matter at ordinary temperatures can be considered to be in ceaseless, random motion at high speeds. The average translational kinetic energy for these molecules can be deduced from the Boltzmann distribution. Knowing the velocity and the temperature of these molecules at different temperatures will allow us to calculate a value for the Molar Mass. The Boltzmann distribution of energies can be broken down to relate average velocities to temperature using the following relation: 3 1 kT = mv 2 2 2 k = 1.38 x 10-23 J/K T in Kelvin m of a single particle in kg v in m/s We can eliminate the 1/2 factor by multiplying both sides by 2 giving us: 3kT = mv 2 y = mx + b You can see how this equation can be viewed and plotted as a linear relationship with v2 as the x-axis and 3kT as the y-axis. PROCEDURE A. Go to the University of Colorado website for science simulations: phet.colorado.edu. 1. Click on the “Play with Simulation” button. 2. Click on “Chemistry” 3. Find the lab the says “Gas Properties” and click on it. 4. You can either use the simulation online or download it as a .jar (Java archive) file. If you click to play and you get a blank screen, you will need to download it. Page 1 of 4 5. Open the .jar file and run it. If you need to install Java on your computer you can do so here https://java.com/en/download/manual.jsp. You may need to restart your computer after installing. B. SETTING UP THE EXPERIMENT 1. Click on “Constant Volume” 2. Click on “Measurement Tools”, then select “Species Information” 3. Click on “Advanced Options” and deselect “Molecules Collide” 4. Record your data from the experiment in the table below for Temperature, Pressure, and Average Speed Heavy Species T(K) Pressure (atm) Average Speed (m/s) Light Species T(K) Pressure (atm) Average Speed (m/s) C. RUNNING THE EXPERIMENT 1. Use the pump handle to pump in between 300 and 600 particles 2. Record the values for the Temperature, Pressure, and Average Speed 3. Use the Heat Control to raise or lower the temperature and record at least 4 additional data points with a total temperature range of at least 500K between the lowest and highest temperatures and at least two below room temperature (300K) 4. Once you are finished recording your data points, click on the “Reset” button to begin a new experiment. (You may need to close the Measurement Tools to find the reset button). 5. Choose the “Light Species” for the Gas in Pump, and repeat steps 1 - 4. Be sure to choose at least one temperature in this series of measurements that is the same as the first series Page 2 of 4 D. DATA ANALYSIS 1. Plot your data as explained in the Introduction for your heavy species and attach to your report. 2. Find the mass of a single particle in kg, and the mass of one mole of particles in g/mol. Show your calculations below. (Note: You will need to find the slope of your line. To find the slope of your line to more than one significant figure in Excel you may need to use the SLOPE function. In a cell type =SLOPE(range of y-values),(range of x-values)) 3. Repeat your analysis for the light species. E. QUESTIONS 1. What is the relationship between temperature and average velocity? Page 3 of 4 2. Using the two measurements that were at the same temperature for the two species, how did the average velocity compare between the heavy and light particles? Explain why this is. 3. How did the pressure respond to the changes in temperature? Explain the reason for this Page 4 of 4

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madushan
School: UT Austin

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