12. Phosphorus pentachloride exists at equilibrium with phosphorus trichloride and chlorine: PCIS → PCla@ + Ca (B) A sample of PCl, with an initial concentration ([PCL) of 3.00 M is placed in an empty container and allowed to react. When the system reaches equilibrium, the concentrations of PCla and Cla are both 1.80 M ([PCL1 = 1.80 M and [Cl] = 1.80 M). a) Calculate the equilibrium concentration of PCl: ([PC:). Show all work. b) Write the equilibrium expression for the reaction above. c) Find the value of the equilibrium constant (K). Show all work. d) Indicate which side of the reaction is favored. Explain how you know. e) Assuming the reaction is endothermic (PCls (2). + Energy PCl3 + Chw), identify two ways in which the equilibrium can be stressed to increase the production of PCl3.

12. Phosphorus pentachloride exists at equilibrium with phosphorus trichloride and chlorine: PCIS → PCla@ + Ca (B) A sample of PCl, with an initial concentration ([PCL) of 3.00 M is placed in an empty container and allowed to react. When the system reaches equilibrium, the concentrations of PCla and Cla are both 1.80 M ([PCL1 = 1.80 M and [Cl] = 1.80 M). a) Calculate the equilibrium concentration of PCl: ([PC:). Show all work. b) Write the equilibrium expression for the reaction above. c) Find the value of the equilibrium constant (K). Show all work. d) Indicate which side of the reaction is favored. Explain how you know. e) Assuming the reaction is endothermic (PCls (2). + Energy PCl3 + Chw), identify two ways in which the equilibrium can be stressed to increase the production of PCl3.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.35PAE: In the reaction in Exercise 12.33, another trial was carried out. The reaction began with an initial...

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