At an elevated temperature, K, = 4.0 × 10-6 for the reaction 2 HBr(g) = H2(g) +Br2(g). If the initial partial pressures of HBr, H2, and Br2 are 1.0 × 10-2 atm, 2.0 × 10-3.4atm, and 2.0 × 10-4 atm, respectively, what is the equilibrium partial pressure of6.H2?At 1000 K, Kp = 19.9 for the reaction Fe203(s) + 3 CO(g) = 2 Fe(s) + 3 CO2(g). Whatis the value of K, for the reaction 4 Fe203(s) + 12 CO(g) = 8 Fe(s) + 12 CO2(g)?Exactly 3.75 moles of N204 is placed in an empty 1.0-L container. After a period oftime, equilibrium is reached and described by the equation below:N204 (g) = 2NO2 (g)If at equilibrium the N204 is 45% dissociated, what is the value of the equilibriumconstant for the reaction? What is the equilibrium equation for the reaction:3NH4NO3(s) = N20(g) + 2 H2O(/)?O A) Ke = [N2O][H2O12%3D6.5-B) Kc = [N20][H2O]8.9.--N20]H20]2Kc%3DNHẠNO3]O D) K = [N20]

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At an elevated temperature, K, = 4.0 × 10-6 for the reaction 2 HBr(g) = H2(g) + Br2(g). If the initial partial pressures of HBr, H2, and Br2 are 1.0 x 10-2 atm, 2.0 × 10- 4 atm, and 2.0 × 10-4 atm, respectively, what is the equilibrium partial pressure of H2?

At an elevated temperature, K, = 4.0 × 10-6 for the reaction 2 HBr(g) = H2(g) + Br2(g). If the initial partial pressures of HBr, H2, and Br2 are 1.0 x 10-2 atm, 2.0 × 10- 4 atm, and 2.0 × 10-4 atm, respectively, what is the equilibrium partial pressure of H2?

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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