Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2( g) + Cl2( g)Δ2 ICl( g) Kp = 81.9 (at 298 K) A reaction mixture at 298 K initially contains PI2 = 0.25 atm and PCl2 = 0.25 atm. What is the partial pressure of iodine monochloride when the reaction reaches equilibrium?a) 0.17 atm b) 0.64 atmc) 0.41 atm d) 2.3 atm
Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2( g) + Cl2( g)Δ2 ICl( g) Kp = 81.9 (at 298 K) A reaction mixture at 298 K initially contains PI2 = 0.25 atm and PCl2 = 0.25 atm. What is the partial pressure of iodine monochloride when the reaction reaches equilibrium?a) 0.17 atm b) 0.64 atmc) 0.41 atm d) 2.3 atm
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
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 3PS: Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A...
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Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2( g) + Cl2( g)Δ2 ICl( g) Kp = 81.9 (at 298 K) A reaction mixture at 298 K initially contains PI2 = 0.25 atm and PCl2 = 0.25 atm. What is the partial pressure of iodine monochloride when the reaction reaches equilibrium?
a) 0.17 atm b) 0.64 atm
c) 0.41 atm d) 2.3 atm
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