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
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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