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

Answered: Image /qna-images/answer/08e112b1-dafe-4373-b6dc-0b3ce6c967f2.jpg

Answered: Phosphorus pentachloride decomposes…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.37PAE: Again the experiment in Exercise 12.33 was redesigned. This time, 0.15 mol each of N, and O2 was...

See similar textbooks

Related questions

Concept explainers

Question

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

Expert Solution

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions