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C. Assuming the reaction takes place in a closed vessel with an initial NO2() 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. D. What will be the equilibrium partial pressure of NO(g) if 2.540 atm of NO2«g) and 0.870 atm of Oz(g) were initially present in the vessel? Show a complete ICE table. Indicate any assumptions that you made in your calculations. E. Calculate the Kp of the reaction at 32 °C given that its AH,xn is –23.40 kJ/mol, with the assumption that AHxn is constant from 20 to 50 °C.

C. Assuming the reaction takes place in a closed vessel with an initial NO2() 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. D. What will be the equilibrium partial pressure of NO(g) if 2.540 atm of NO2«g) and 0.870 atm of Oz(g) were initially present in the vessel? Show a complete ICE table. Indicate any assumptions that you made in your calculations. E. Calculate the Kp of the reaction at 32 °C given that its AH,xn is –23.40 kJ/mol, with the assumption that AHxn is constant from 20 to 50 °C.

Chemistry
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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Please answer part c, d and e. The answer for a and b is as follows: 

a. 9.75×10^-7 
b. 4.82×10^−6

1. Consider the decomposition reaction shown below. NO2(8) 2 NO(g) + ½ O2(g) A. What is the equilibrium constant (Kc) of the above reaction at 25 °C given that its AG°xn 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 NO2(e) 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. D. What will be the equilibrium partial pressure of NOe) if 2.540 atm of NOz(e) and 0.870 atm of O2(g) were initially present in the vessel? Show a complete ICE table. Indicate any assumptions that you made in your calculations. E. Calculate the Kp of the reaction at 32 °C given that its AHxn is –23.40 kJ/mol, with the assumption that AHrxn is constant from 20 to 50 °C.
Transcribed Image Text:1. Consider the decomposition reaction shown below. NO2(8) 2 NO(g) + ½ O2(g) A. What is the equilibrium constant (Kc) of the above reaction at 25 °C given that its AG°xn 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 NO2(e) 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. D. What will be the equilibrium partial pressure of NOe) if 2.540 atm of NOz(e) and 0.870 atm of O2(g) were initially present in the vessel? Show a complete ICE table. Indicate any assumptions that you made in your calculations. E. Calculate the Kp of the reaction at 32 °C given that its AHxn is –23.40 kJ/mol, with the assumption that AHrxn is constant from 20 to 50 °C.
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