2NOCI(g) = 2NO(g) + Cl₂(g) K = 1.6 x 10-5 @ 35°C K = [NO]²[C1₂] [NOCI]2 Calculate the equilibrium concentrations of the gases if the reaction begins with 3.0 moles of NOCI in a 2.0 L flask. What is the concentration of NO? [NO]=[?] x 10) M Coefficient (green) -2 Exponent (yellow) Enter
2NOCI(g) = 2NO(g) + Cl₂(g) K = 1.6 x 10-5 @ 35°C K = [NO]²[C1₂] [NOCI]2 Calculate the equilibrium concentrations of the gases if the reaction begins with 3.0 moles of NOCI in a 2.0 L flask. What is the concentration of NO? [NO]=[?] x 10) M Coefficient (green) -2 Exponent (yellow) Enter
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 1PS: Write equilibrium constant expressions for the following reactions. For gases, use either pressures...
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I still keep getting this question wrong. I put 4.2 E -2 as my answer, and it says I'm correct. So then, I tried 4.16 E -2, then 4.1 E-2, but it still didn't work. I am incredibly lost in this assignment. What am I doing wrong?
![2NOCI(g) = 2NO(g) + Cl₂(g)
K = 1.6 x 10-5 @ 35°C K = [NO]²[₂]
[NOCI2
Calculate the equilibrium concentrations of
the gases if the reaction begins with
3.0 moles of NOCI in a 2.0 L flask. What is
the concentration of NO?
[NO]=[?] x 10 M
Coefficient (green)
-2
Exponent (yellow)
Enter](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd1e3d50a-9484-42c0-9488-860c281047e5%2F5aa173d1-cd32-4752-8ee6-31fdecc6e43a%2Fmaljztn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:2NOCI(g) = 2NO(g) + Cl₂(g)
K = 1.6 x 10-5 @ 35°C K = [NO]²[₂]
[NOCI2
Calculate the equilibrium concentrations of
the gases if the reaction begins with
3.0 moles of NOCI in a 2.0 L flask. What is
the concentration of NO?
[NO]=[?] x 10 M
Coefficient (green)
-2
Exponent (yellow)
Enter
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