please help with both, will upvote 1] me CH₂Cl₂ is placed in a sealed flask and heated to 408 K. When equilibrium is reached, the flask is found to contain CH₂Cl₂ (1.16×10-2 M), CH4 (1.77x10-2 M), and CCl4 (3.20x10-2 M). What is the value of the equilibrium constant for this reaction at 408 K? 2CH₂Cl₂(g) CH4(g) + CCl4(g) K = 2] Question Content Area The equilibrium constant, K, for the following reaction is 1.29x10-² at 600 K. CoCl₂(g) = CO(g) + Cl2₂(g) If an equilibrium mixture of the three gases in a 12.3 L container 600 K contains 0.459 mol of COCl₂(g) and 0.388 mol of CO, the equilibrium concentration of Cl₂ is M.
please help with both, will upvote 1] me CH₂Cl₂ is placed in a sealed flask and heated to 408 K. When equilibrium is reached, the flask is found to contain CH₂Cl₂ (1.16×10-2 M), CH4 (1.77x10-2 M), and CCl4 (3.20x10-2 M). What is the value of the equilibrium constant for this reaction at 408 K? 2CH₂Cl₂(g) CH4(g) + CCl4(g) K = 2] Question Content Area The equilibrium constant, K, for the following reaction is 1.29x10-² at 600 K. CoCl₂(g) = CO(g) + Cl2₂(g) If an equilibrium mixture of the three gases in a 12.3 L container 600 K contains 0.459 mol of COCl₂(g) and 0.388 mol of CO, the equilibrium concentration of Cl₂ is M.
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...
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![please help with both, will upvote
1] me CH₂Cl₂ is placed in a sealed flask and heated to 408 K. When equilibrium is reached, the flask is found to contain CH₂Cl₂ (1.16×10-² M), CH4 (1.77×10-² M), and CCl4
(3.20x10-2 M). What is the value of the equilibrium constant for this reaction at 408 K?
2CH₂Cl₂(g) CH4(g) + CCl4(g) K=
2]
Question Content Area
The equilibrium constant, K, for the following reaction is 1.29x10-2 at 600 K.
CoCl₂(g) = CO(g) + Cl₂(g)
If an equilibrium mixture of the three gases in a 12.3 L container at 600 K contains 0.459 mol of COCI₂(g) and 0.388 mol of CO, the equilibrium concentration of Cl₂ is M.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F910f8be2-fbed-42ae-8bd1-d6d675c4531a%2Faa3e2a53-4965-48bb-917f-5f0140b4e770%2F0v7qkul_processed.png&w=3840&q=75)
Transcribed Image Text:please help with both, will upvote
1] me CH₂Cl₂ is placed in a sealed flask and heated to 408 K. When equilibrium is reached, the flask is found to contain CH₂Cl₂ (1.16×10-² M), CH4 (1.77×10-² M), and CCl4
(3.20x10-2 M). What is the value of the equilibrium constant for this reaction at 408 K?
2CH₂Cl₂(g) CH4(g) + CCl4(g) K=
2]
Question Content Area
The equilibrium constant, K, for the following reaction is 1.29x10-2 at 600 K.
CoCl₂(g) = CO(g) + Cl₂(g)
If an equilibrium mixture of the three gases in a 12.3 L container at 600 K contains 0.459 mol of COCI₂(g) and 0.388 mol of CO, the equilibrium concentration of Cl₂ is M.
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