A student placed 0.264 mol of PCI3(g) and 0.180 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction PCI3(3) + Cl2(3) = 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

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What were the equilibrium concentrations?
The equilibrium concentration of PCI3 =
i
M
The equilibrium concentration of Cl2 =
i
%3D
The equilibrium concentration of PCI5 =
M
What is the value of K. for this reaction at this temperature?
K =
Transcribed Image Text:What were the equilibrium concentrations? The equilibrium concentration of PCI3 = i M The equilibrium concentration of Cl2 = i %3D The equilibrium concentration of PCI5 = M What is the value of K. for this reaction at this temperature? K =
A student placed 0.264 mol of PCI3(g) and 0.180 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction
PCI3(3) + Cl2(g)Z 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] =
M
[PCI5] =
M
i
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
M
The concentration of PCI5 has increased by
M
Transcribed Image Text:A student placed 0.264 mol of PCI3(g) and 0.180 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction PCI3(3) + Cl2(g)Z 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] = M [PCI5] = M i 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 M The concentration of PCI5 has increased by M
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