Given: PCI5(g) What would be the equilibrium concentration of PCI5(g) if 0.20 mole of PCI5(g) was placed in a 1.00-L container at this temperature? What would be the new equilibrium concentration of PCI5(g) if the volume vere halved at this same temperature? = PCI3(g) + Cl2(g) Kc = 0.040 at 450°C
Given: PCI5(g) What would be the equilibrium concentration of PCI5(g) if 0.20 mole of PCI5(g) was placed in a 1.00-L container at this temperature? What would be the new equilibrium concentration of PCI5(g) if the volume vere halved at this same temperature? = PCI3(g) + Cl2(g) Kc = 0.040 at 450°C
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 38A
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Question
![Given: PCI5(g)
= PCl:(g) + Cl2(g)
Kc = 0.040 at 450°C
What would be the equilibrium concentration of PCI5(g) if 0.20 mole of
PCI5(g) was placed in a 1.00-L container at this temperature?
What would be the new equilibrium concentration of PCI5(g) if the volume
were halved at this same temperature?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F24bc21c6-fcf3-4a23-b63f-4d84d4d4c613%2F3f945772-b302-4e2a-923d-89a02e068c36%2Fjdtijts_processed.png&w=3840&q=75)
Transcribed Image Text:Given: PCI5(g)
= PCl:(g) + Cl2(g)
Kc = 0.040 at 450°C
What would be the equilibrium concentration of PCI5(g) if 0.20 mole of
PCI5(g) was placed in a 1.00-L container at this temperature?
What would be the new equilibrium concentration of PCI5(g) if the volume
were halved at this same temperature?
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