1. Consider the decomposition reaction shown below. NO2(g) 2 NO(g) + ½ O2(g) A. What is the equilibrium constant (Kc) of the above reaction at 25 °C given that its AG°rn is +34.85 kJ/mol at this temperature? B. Calculate the Kp of the reaction at 25 °C. C. Assuming the reaction takes place in a closed vessel with an initial NO2e) pressure of 2.540 atm, what are the partial pressures of each of the gases at equilibrium? Show a complete ICE table. Indicate any assumptions that you made in your calculations.

1. Consider the decomposition reaction shown below. NO2(g) 2 NO(g) + ½ O2(g) A. What is the equilibrium constant (Kc) of the above reaction at 25 °C given that its AG°rn is +34.85 kJ/mol at this temperature? B. Calculate the Kp of the reaction at 25 °C. C. Assuming the reaction takes place in a closed vessel with an initial NO2e) pressure of 2.540 atm, what are the partial pressures of each of the gases at equilibrium? Show a complete ICE table. Indicate any assumptions that you made in your calculations.

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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