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
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![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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0fbb3c06-e00f-403d-b22e-2085aedad23d%2Fe45e0a5b-73d4-4c7f-ae86-f199a6335ef0%2Fwusso5d_processed.png&w=3840&q=75)
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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