This is my second time asking this question, the first one came out as incorrect for both answers (I attached pictures of answers). I'm not sure what is done incorrectly. Phosphorus pentachloride decomposes according to the chemical equationPCl5(g)↽−−⇀PCl3(g)+Cl2(g) ?c=1.80 at 250 A 0.2738 mol sample of PCl5⁢(g) is injected into an empty 3.90 L reaction vessel held at 250⁢ ∘C.Calculate the concentrations of PCl5⁢(g) and PCl3(g) at equilibrium. Phosphorus pentachloride decomposes according to the chemical equationPCI, (g) = PCI, (g) + Cl, (g)K. = 1.80 at 250 °CA 0.2738 mol sample of PCl, (g) is injected into an empty 3.90 L reaction vessel held at 250 °C.Calculate the concentrations of PCl, (g) and PCl, (g) at equilibrium.0.00716[PCI,] =|MIncorrect0.00716[PCI,] =MIncorrect Let's put these values into the equilibrium constant formula:[PCI,]K.[PC!3] [Clz]= 1.800.070205 – x= 1.80х20.070205 – x = 1.80 x²-1.80 x? + x – 0.070205By solving the above quadratic equation, we get:x = 0.063049Final answerThe equilibrium concentration of PCI5 is given by:PCI5g = 0.070205 -XPC158 = 0.070205 -0.063049PC158 = 0.007156 MPCI5(g) = 0.00716 MThe equilibrium concentration of PCI3 is given by:PC13g = XPC139 = 0.063049 MPCI3(g) = 0.0630 M

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Answered: Phosphorus pentachloride decomposes…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.86QE

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This is my second time asking this question, the first one came out as incorrect for both answers (I attached pictures of answers). I'm not sure what is done incorrectly.

Phosphorus pentachloride decomposes according to the chemical equation

PCl5(g)↽−−⇀PCl3(g)+Cl2(g) ?c=1.80 at 250

A 0.2738 mol sample of PCl5⁢(g) is injected into an empty 3.90 L reaction vessel held at 250⁢ ∘C.

Calculate the concentrations of PCl5⁢(g) and PCl3(g) at equilibrium.

Phosphorus pentachloride decomposes according to the chemical equation
PCI, (g) = PCI, (g) + Cl, (g)
K. = 1.80 at 250 °C
A 0.2738 mol sample of PCl, (g) is injected into an empty 3.90 L reaction vessel held at 250 °C.
Calculate the concentrations of PCl, (g) and PCl, (g) at equilibrium.
0.00716
[PCI,] =|
M
Incorrect
0.00716
[PCI,] =
M
Incorrect

Let's put these values into the equilibrium constant formula:
[PCI,]
K.
[PC!3] [Clz]
= 1.80
0.070205 – x
= 1.80
х2
0.070205 – x = 1.80 x²
-
1.80 x? + x – 0.070205
By solving the above quadratic equation, we get:
x = 0.063049
Final answer
The equilibrium concentration of PCI5 is given by:
PCI5g = 0.070205 -XPC158 = 0.070205 -0.063049PC158 = 0.007156 MPCI5(g) = 0.00716 M
The equilibrium concentration of PCI3 is given by:
PC13g = XPC139 = 0.063049 MPCI3(g) = 0.0630 M

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