A student placed O.236 mol of PCI3(g) and 0.145 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction PCI3(3) + Cl2(g) 2 PCI5(g) came to equilibrium it was found that the flask contained 0.120 mol of PCI3. What were the initial concentrations of the reactants and product? [PCI3] = i M [Cl2] = i M [PCI5) = i M
A student placed O.236 mol of PCI3(g) and 0.145 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction PCI3(3) + Cl2(g) 2 PCI5(g) came to equilibrium it was found that the flask contained 0.120 mol of PCI3. What were the initial concentrations of the reactants and product? [PCI3] = i M [Cl2] = i M [PCI5) = i M
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 51QRT: At room temperature, the equilibrium constant Kc for the reaction
2 NO(g) ⇌ N2(g) + O2(g)
is 1.4 ×...
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A student placed 0.236 mol of PCl3(g) and 0.145 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction
PCl3(g) + Cl2(g) ⇄ PCl5(g) came to equilibrium it was found that the flask contained 0.120 mol of PCl3.
![A student placed O.236 mol of PCI3(g) and 0.145 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction
PCI3(3) + Cl2(g) 2 PCI5(g) came to equilibrium it was found that the flask contained 0.120 mol of PCI3.
What were the initial concentrations of the reactants and product?
[PCI3] = i
M
[Cl2] = i
M
[PCI5) = i
M
By how much had the concentrations changed when the reaction reached equilibrium?
The concentration of PCI3 has decreased by i
M
The concentration of Cl2 has decreased by i
M
The concentration of PCI5 has increased by i
M
What were the equilibrium concentrations?
The equilibrium concentration of PCI3 = i
M
The equilibrium concentration of Cl2 = i
M
The equilibrium concentration of PCI5 = i
M
What is the value of K. for this reaction at this temperature?
K =](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fef4c261e-ab8b-4e31-87b0-53d74058044a%2Fd67a06dc-ca8b-4e3c-aa55-1b9a113e9b9f%2Fnm4uqi_processed.png&w=3840&q=75)
Transcribed Image Text:A student placed O.236 mol of PCI3(g) and 0.145 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction
PCI3(3) + Cl2(g) 2 PCI5(g) came to equilibrium it was found that the flask contained 0.120 mol of PCI3.
What were the initial concentrations of the reactants and product?
[PCI3] = i
M
[Cl2] = i
M
[PCI5) = i
M
By how much had the concentrations changed when the reaction reached equilibrium?
The concentration of PCI3 has decreased by i
M
The concentration of Cl2 has decreased by i
M
The concentration of PCI5 has increased by i
M
What were the equilibrium concentrations?
The equilibrium concentration of PCI3 = i
M
The equilibrium concentration of Cl2 = i
M
The equilibrium concentration of PCI5 = i
M
What is the value of K. for this reaction at this temperature?
K =
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