(a) Calculate the equilibrium partial pressures of O2, NOCl, NO2, and Cl2. Peq(O2) = . Peq(NOCl) = . Peq(NO2) = . Peq(Cl2) = . (b) Calculate KP for this reaction
(a) Calculate the equilibrium partial pressures of O2, NOCl, NO2, and Cl2. Peq(O2) = . Peq(NOCl) = . Peq(NO2) = . Peq(Cl2) = . (b) Calculate KP for this reaction
Introductory Chemistry: A Foundation
8th Edition
ISBN:9781285199030
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 20QAP
Related questions
Question
A mixture of 0.1242 mol of O2, 0.1313 mol of NOCl, 0.1522 mol of NO2, and 0.1981 mol of Cl2 is placed in a 1.0-L steel pressure vessel at 565 K. The following equilibrium is established:
1 O2(g) + 2 NOCl(g) 2 NO2(g) + 1 Cl2(g)
At equilibrium 0.08054 mol of O2 is found in the reaction mixture.
(a) Calculate the equilibrium partial pressures of O2, NOCl, NO2, and Cl2.
Peq(O2) = .
Peq(NOCl) = .
Peq(NO2) = .
Peq(Cl2) = .
(b) Calculate KP for this reaction.
KP = .
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