Consider the following equilibrium process at 686. °C: CO₂(g) + H₂(g) CO(g) + H₂O(g) The equilibrium concentrations of the reacting species are [CO]= 0.0550 M, [H₂] = 0.0400 M, [CO₂] = 0.0820 M, and [H₂O]=0.0400 M. Part 1 of 5 Calculate K for the reaction at 686. °C. Be sure your answer has the correct number of significant digits. K= Part 2 of 5 0 x10 x If we add CO₂ to increase its concentration to 0.430 M, what will the concentrations of all the gases be when equilibrium is reestablished? Be sure your answer has the correct number of significant digits. [CO₂] = M 7.9
Consider the following equilibrium process at 686. °C: CO₂(g) + H₂(g) CO(g) + H₂O(g) The equilibrium concentrations of the reacting species are [CO]= 0.0550 M, [H₂] = 0.0400 M, [CO₂] = 0.0820 M, and [H₂O]=0.0400 M. Part 1 of 5 Calculate K for the reaction at 686. °C. Be sure your answer has the correct number of significant digits. K= Part 2 of 5 0 x10 x If we add CO₂ to increase its concentration to 0.430 M, what will the concentrations of all the gases be when equilibrium is reestablished? Be sure your answer has the correct number of significant digits. [CO₂] = M 7.9
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 66QAP: Consider the equilibrium H2(g)+S(s)H2S(g)When this system is at equilibrium at 25C in a 2.00-L...
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[H2]= .....M
[CO]= ...M
[H2O]=....M
![Consider the following equilibrium process at 686. °℃:
CO₂(g) + H₂(g) ⇒ CO(g) + H₂O(g)
The equilibrium concentrations of the reacting species are [CO]=0.0550 M, [H₂] = 0.0400 M, [CO₂] = 0.0820 M, and [H₂O] = 0.0400 M.
Part 1 of 5
Calculate K for the reaction at 686. °C. Be sure your answer has the correct number of significant digits.
K=
=
Part 2 of 5
x10
x
Ś
If we add CO₂ to increase its concentration to 0.430 M, what will the concentrations of all the gases be when equilibrium is reestablished?
Be sure your answer has the correct number of significant digits.
[CO₂] = M
10](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3f33cc2f-0221-41a8-a3a2-cc96bc7960a2%2F5f2fbcd4-0543-4c3f-9132-e01af768dce4%2F6dne4u_processed.png&w=3840&q=75)
Transcribed Image Text:Consider the following equilibrium process at 686. °℃:
CO₂(g) + H₂(g) ⇒ CO(g) + H₂O(g)
The equilibrium concentrations of the reacting species are [CO]=0.0550 M, [H₂] = 0.0400 M, [CO₂] = 0.0820 M, and [H₂O] = 0.0400 M.
Part 1 of 5
Calculate K for the reaction at 686. °C. Be sure your answer has the correct number of significant digits.
K=
=
Part 2 of 5
x10
x
Ś
If we add CO₂ to increase its concentration to 0.430 M, what will the concentrations of all the gases be when equilibrium is reestablished?
Be sure your answer has the correct number of significant digits.
[CO₂] = M
10
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