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
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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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![12. Phosphorus pentachloride exists at equilibrium with phosphorus
trichloride and chlorine:
PCI5 (2) = PCla + Clae
A sample of POCI, with an initial concentration ([PCL) of 3.00M 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 ([PCL] = 1.80 M and [Cl] = 1.80 M).
a) Calculate the equilibrium concentration of PCl: ([PCL). 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 PCae
+ Chw),
identify two ways in which the equilibrium can be stressed to increase the production
of PCla.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F568f6bdd-bb57-4ef6-85de-b375d9807015%2F01a6ca44-ead3-454a-a55a-112b1a1d95ab%2Fwm5i61c_processed.jpeg&w=3840&q=75)
Transcribed Image Text:12. Phosphorus pentachloride exists at equilibrium with phosphorus
trichloride and chlorine:
PCI5 (2) = PCla + Clae
A sample of POCI, with an initial concentration ([PCL) of 3.00M 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 ([PCL] = 1.80 M and [Cl] = 1.80 M).
a) Calculate the equilibrium concentration of PCl: ([PCL). 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 PCae
+ Chw),
identify two ways in which the equilibrium can be stressed to increase the production
of PCla.
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