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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Answered: (a) Calculate the equilibrium partial…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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.

P_eq(O₂) =  .

P_eq(NOCl) =  .

P_eq(NO₂) =  .

P_eq(Cl₂) =  .

(b) Calculate K_P for this reaction.

K_P =  .