0.150 mol of COCl2(g) sealed in a volume of 10.0 L forms CO(g) and Cl2(g) at 360 °C. Use K = 8.3×10–4 M to find all [conc]eq in this equilibrium mixture: COCl2(g) <--> Cl2(g) + CO(g) K= ------- = 8.3x10-4 Set up ICE Table. Use other given data to calculate the unknown: K = -------- = 8.3x10-4 __x2 + _______ x _______ = 0 (b2–4ac)½ = _______ x=______________ = ______ x=______________ = ______
0.150 mol of COCl2(g) sealed in a volume of 10.0 L forms CO(g) and Cl2(g) at 360 °C. Use K = 8.3×10–4 M to find all [conc]eq in this equilibrium mixture: COCl2(g) <--> Cl2(g) + CO(g) K= ------- = 8.3x10-4 Set up ICE Table. Use other given data to calculate the unknown: K = -------- = 8.3x10-4 __x2 + _______ x _______ = 0 (b2–4ac)½ = _______ x=______________ = ______ x=______________ = ______
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
Section15.3: Determining An Equilibrium Constant
Problem 15.3CYU: A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent...
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0.150 mol of COCl2(g) sealed in a volume of 10.0 L forms CO(g) and Cl2(g) at 360 °C. Use K = 8.3×10–4 M to find all [conc]eq in this equilibrium mixture:
COCl2(g) <--> Cl2(g) + CO(g) K= ------- = 8.3x10-4
Set up ICE Table.
Use other given data to calculate the unknown:
K = -------- = 8.3x10-4
__x2 + _______ x _______ = 0
(b2–4ac)½ = _______
x=______________ = ______
x=______________ = ______
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