You are interested in finding out the magnitude of the devia…
You are interested in finding out the magnitude of the deviations from ideal gas behavior by comparing the results of calculations using the ideal gas equation and the van der Waals equation for 1.00 mole of CO2 at 0oC in containers of different volumes. Let’s start with a 22.4 L container.van der Waals Constants for CO2a = 3.592 L2-atm/mol2 b = 0.04267 L/mol Part A. 2 pointsWhat is the pressure of this gas if we treat it as an ideal gas? Part B. 2 pointsWhat is the pressure of this gas if we treat it as real? Part C. 2 pointsLet’s now repeat this calculation, assuming that the gas is compressed so that it fills a container that has a volume of only 0.200 liters. What is the pressure now if we treat it as an ideal gas? Part D. 2 pointsWhat is the pressure in scenario C, if we treat the gas as real? Part E. 2 points Let’s now compress the gas even further, raising the pressure until the volume of the gas is only 0.0500 liters. What is the pressure if we treat the gas as ideal? Part F. 2 points What is the pressure if we treat the gas in part E as real? Part G. 5 pointsShown below is a plot of the product of the pressure times the volume for samples of CO2 gas versus the pressure. What would you expect this graph to look like for an ideal gas by comparison? Figure: pressure p vs the product of p*V for CO2 gas Feel free to sketch or describe your answer. Part H. 5 pointsWhat is a plausible interpretation for the results obtained in parts A-G? Solve this problem on paper, document your approach and provide intermediate results. Report the final answers with 3 significant figures. Scan the pages(s) and upload them for grading. Complete all parts A-H.