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The total pressure of the following system is used to monitor the progress of the chemical reaction. SO₂Cl(g) → SO(g) + Cla(g) The reaction is initiated, and the following data are obtained: 0 3 6 Time (h) 9 12 15 20.71 Potal (kPa) 11.07 14.79 17.26 18.90 19.99 Pso₂Cl₂ Pso₂ Pcl₂ Additional information: As the reaction proceeds, stoichiometry dictates that for every mole of SO,Cl; that dissociates one mole of each of SO₂ and Cl₂ is produced. Defining the extent of dissociation/reaction as , and the initial pressure as Po, the total pressure is given by: Ptotal= Pso,cl, + Pso,+Pa,= (Po-5)+5+5 a) Calculate the pressure of each component at each time interval, i.e. complete the above table. b) Use a graphical method and determine what the order of the reaction is with respect to SO,Cl₂? (i) Show the plot as well as the linear fit of the data. (ii) Motivate your answer. c) Determine the rate constant for this reaction.

The total pressure of the following system is used to monitor the progress of the chemical reaction. SO₂Cl(g) → SO(g) + Cla(g) The reaction is initiated, and the following data are obtained: 0 3 6 Time (h) 9 12 15 20.71 Potal (kPa) 11.07 14.79 17.26 18.90 19.99 Pso₂Cl₂ Pso₂ Pcl₂ Additional information: As the reaction proceeds, stoichiometry dictates that for every mole of SO,Cl; that dissociates one mole of each of SO₂ and Cl₂ is produced. Defining the extent of dissociation/reaction as , and the initial pressure as Po, the total pressure is given by: Ptotal= Pso,cl, + Pso,+Pa,= (Po-5)+5+5 a) Calculate the pressure of each component at each time interval, i.e. complete the above table. b) Use a graphical method and determine what the order of the reaction is with respect to SO,Cl₂? (i) Show the plot as well as the linear fit of the data. (ii) Motivate your answer. c) Determine the rate constant for this reaction.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The total pressure of the following system is used to monitor the progress of the chemical reaction. SO₂Cl2(g) → SO2(g) + Cl.(g) The reaction is initiated, and the following data are obtained: 3 6 0 9 12 Time (h) 15 17.26 18.90 19.99 20.71 PTotal (kPa) 11.07 14.79 Pso₂Cl₂ Pso₂ Pcl₂ Additional information: As the reaction proceeds, stoichiometry dictates that for every mole of SO₂Cl₂ that dissociates one mole of each of SO₂ and Cl₂ is produced. Defining the extent of dissociation/reaction as, and the initial pressure as Po, the total pressure is given by: Ptotal = Pso₂Cl₂ + Pso₂+ Pal₂ = (Po-5)+5+5 a) Calculate the pressure of each component at each time interval, i.e. complete the above table. b) Use a graphical method and determine what the order of the reaction is with respect to SO,Cl₂? (i) Show the plot as well as the linear fit of the data. (ii) Motivate your answer. c) Determine the rate constant for this reaction.
Transcribed Image Text:The total pressure of the following system is used to monitor the progress of the chemical reaction. SO₂Cl2(g) → SO2(g) + Cl.(g) The reaction is initiated, and the following data are obtained: 3 6 0 9 12 Time (h) 15 17.26 18.90 19.99 20.71 PTotal (kPa) 11.07 14.79 Pso₂Cl₂ Pso₂ Pcl₂ Additional information: As the reaction proceeds, stoichiometry dictates that for every mole of SO₂Cl₂ that dissociates one mole of each of SO₂ and Cl₂ is produced. Defining the extent of dissociation/reaction as, and the initial pressure as Po, the total pressure is given by: Ptotal = Pso₂Cl₂ + Pso₂+ Pal₂ = (Po-5)+5+5 a) Calculate the pressure of each component at each time interval, i.e. complete the above table. b) Use a graphical method and determine what the order of the reaction is with respect to SO,Cl₂? (i) Show the plot as well as the linear fit of the data. (ii) Motivate your answer. c) Determine the rate constant for this reaction.
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