UNIT 4 IB MATERIAL Name: PARTICLE BEHAVIOR OF MATTER PHASES & ATTRACTIONS ESSENTIALS: Know, Understand, and Be Able To Apply Avogadro s law to calculate reacting volumes of gases. Apply the concept of molar volume at standard temperature and pressure in calculations. Solve problems involving the relationship between temperature, pressure, and volume for a fixed mass of an ideal gas. Solve problems using the ideal gas equation, PV = nrt Analyse graphs relating to the ideal gas equation. Describe the kinetic theory in terms of the movement of particles whose average energy is proportional to temperature in kelvins. Describe the collision theory (more next unit). IB Study Guide Page References: p. 10-11 ELABORATE Assignments ENVISION TOK Question on Moodle forum EVALUATE IB portion on Unit Test
Assignment:
Assignment:
Assignment: Ideal Gas Law Practice Directions: Solve the following problems. Be sure to write the equation used and show how numbers were put into the equation. All answers must have the correct units. 1. If 4.27 moles of propane are at a temperature of 33.79 oc and are under 167.98 kpa of pressure, what volume does the sample occupy? 2. A sample of carbon monoxide at 55.68 oc and under 0.2 atm of pressure takes up 67.12 L of space. What mass of carbon monoxide is present in the sample? 3. At -41.3 oc, 42.06 g of fluorine gas take up 2,788.91 ml of space. What is the pressure of the gas, in kpa? 4. At 758.85 mm Hg, 238.96 g of carbon dioxide have a volume of 65.45 dm3. What is the temperature of the sample, in oc? 5. At 137 oc and under a pressure of 3.11 atm, a 276 g sample of an unknown noble gas occupies 13.46 L of space. What is the gas?
Assignment: More Ideal Gas Law Practice (if needed) Directions: Solve the following problems. Be sure to write the equation used and show how numbers were put into the equation. All answers must have the correct units. 1. If 4.32 moles of propane are at a temperature of 56.25 oc and are under 273.61 kpa of pressure, what volume does the sample occupy? 2. A sample of carbon monoxide at 73.34 oc and under 0.61 atm of pressure takes up 80.39 L of space. What mass of carbon monoxide is present in the sample? 3. At -31.31 oc, 69.29 g of fluorine gas take up 1,236.21 ml of space. What is the pressure of the gas, in kpa? 4. At 679.57 mm Hg, 410.01 g of carbon dioxide have a volume of 24.14 dm3. What is the temperature of the sample, in oc? 5. At 137 oc and under a pressure of 3.11 atm, a 276 g sample of an unknown noble gas occupies 13.46 L of space. What is the gas?
Assignment: Dalton s Law of Partial Pressures Dalton s Law Problems 1. A mixture of neon and argon gases exerts a total pressure of 2.39 atm. The partial pressure of the neon alone is 1.84 atm. What is the partial pressure of the argon? 2. What is the partial pressure of water vapor in an air sample when the total pressure is 1.00 atm, the partial pressure of nitrogen ins 0.79 atm, the partial pressure of oxygen is 0.20 atm and the partial pressure of all other gases in air is 0.00044 atm? 3. What is the total gas pressure in a sealed flask that contains oxygen at a partial pressure of 0.41 atm and water vapor at a partial pressure of 0.58 atm? 4. Find the partial pressure of oxygen in a sealed vessel that has a total pressure of 2.6 atm and also contains carbon dioxide at 1.3 atm and helium at 0.22 atm. 5. A 450 cm 3 sample of H 2 is collected over water at 10 C. The pressure of the H 2 and water vapor is 78.5 kpa. What is the partial pressure of the dry H 2 gas? (watch out for the extra information in this problem and don t forget to use that table in your notes).
Assignment: Maxwell-Boltzmann Distribution The three lines on the graph are the same gas (both type and amount) for different temperatures. I will refer to them as either solid, (-100), dashed (20) and dotted (600). The Y-axis is the number of molecules that have a given speed. 1) Why is speed equivalent to temperature? 2) Do all molecules at the same temperature a. have the same speed? Y/N b. have the same average speed? Y/N 3) State three differences in the size/shape of the curve for higher temperatures.
4) How many molecules have the following speeds: Speed Number of gas particles (SOLID LINE) Number of gas particles (DASHED LINE) Number of gas particles (DOTTED LINE) 200 400 600 5) Will the area under the solid line = the area under the dashed line? Will either equal the area under the dotted line? 6) Draw slanted lines in the area that corresponds to all the molecules that have speeds of 600 m/s or greater for the solid line graph. 7) Using a different kind of shading (slanted lines the other direction, etc.), show all the molecules that have speeds of 600 m/s or greater for the dashed lines and dotted lines. 8) Which temperature has the most molecules with speeds above 600 m/s?