Phosphorus pentachloride decomposes at higher temperatures. PCI5(g) PCI3(g) + Cl2(g) An equilibrium mixture at some temperature consists of 4.66 g PCI5, 208.23 g/mol 4.86 g PCI3, 137.33 g/mol 3.59 g Cl,, 70.91 g/mol in a 1.00-L flask. If you add 1.31g of Cl,, how will the equilibrium be affected and what will the concentration of PCI, be when equilibrium is reestablished? O shift left O shift right O no shift will occur [PCI5] = mol/L Submit Show Approach Show Tutor Steps
Phosphorus pentachloride decomposes at higher temperatures. PCI5(g) PCI3(g) + Cl2(g) An equilibrium mixture at some temperature consists of 4.66 g PCI5, 208.23 g/mol 4.86 g PCI3, 137.33 g/mol 3.59 g Cl,, 70.91 g/mol in a 1.00-L flask. If you add 1.31g of Cl,, how will the equilibrium be affected and what will the concentration of PCI, be when equilibrium is reestablished? O shift left O shift right O no shift will occur [PCI5] = mol/L Submit Show Approach Show Tutor Steps
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 43GQ: Phosphorus pentachloride decomposes at elevated temperatures. PCl5(g) PCl3(g) + Cl2(g) An...
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![Phosphorus pentachloride decomposes at higher temperatures.
PCI5(g) PCI3(g) + Cl2(g)
An equilibrium mixture at some temperature consists of
4.66 g PCI5, 208.23 g/mol
4.86 g PCI3, 137.33 g/mol
3.59 g Cl,, 70.91 g/mol
in a 1.00-L flask.
If you add 1.31g of Cl,, how will the equilibrium be affected and what will the concentration of PCI, be when equilibrium is reestablished?
O shift left
O shift right
O no shift will occur
[PCI5] =
mol/L
Submit
Show Approach Show Tutor Steps](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F445178e5-eb66-4a17-8b6f-493656b3ff53%2Feaef2834-78d0-43ec-a609-d6fcee47653a%2Fduw3b92_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Phosphorus pentachloride decomposes at higher temperatures.
PCI5(g) PCI3(g) + Cl2(g)
An equilibrium mixture at some temperature consists of
4.66 g PCI5, 208.23 g/mol
4.86 g PCI3, 137.33 g/mol
3.59 g Cl,, 70.91 g/mol
in a 1.00-L flask.
If you add 1.31g of Cl,, how will the equilibrium be affected and what will the concentration of PCI, be when equilibrium is reestablished?
O shift left
O shift right
O no shift will occur
[PCI5] =
mol/L
Submit
Show Approach Show Tutor Steps
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