For the equilibrium 3H₂(g) + PMH, -0.00239 atm, P,-0.763 atm and P,-0.921 atm, at 500°C. Calculate Kp. N₂(g)2NH₂(g), the equilibrium partial pressures are For the equilibrium 2NO(g) + 3H₂O2(g) --> 2NH3(g) + 402(g) Kp= 0.244 at 1400 K. When the partial pressures of the gases are PNO= 0.0382 atm, PH202 = 0.0974 atm, PNH3 = 0.264 atm, and Po2 = 0.126 atm, based on the reaction quotient (Q) which direction would the reaction proceed to reach equilibrium? (left or right)

For the equilibrium 3H₂(g) + PMH, -0.00239 atm, P,-0.763 atm and P,-0.921 atm, at 500°C. Calculate Kp. N₂(g)2NH₂(g), the equilibrium partial pressures are For the equilibrium 2NO(g) + 3H₂O2(g) --> 2NH3(g) + 402(g) Kp= 0.244 at 1400 K. When the partial pressures of the gases are PNO= 0.0382 atm, PH202 = 0.0974 atm, PNH3 = 0.264 atm, and Po2 = 0.126 atm, based on the reaction quotient (Q) which direction would the reaction proceed to reach equilibrium? (left or right)

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

For the equilibrium 3H₂(g) + N₂(g) 2NH3(g), the equilibrium partial pressures are
PNH, -0.00239 atm, P,-0.763 atm and P,-0.921 atm, at 500°C. Calculate Kp.
For the equilibrium
2NO(g) + 3H₂O2(g) --> 2NH3(g) + 402(g)
Kp= 0.244 at 1400 K.
When the partial pressures of the gases are PNO = 0.0382 atm, PH202 = 0.0974 atm, PNH3 = 0.264
atm, and Po2 = 0.126 atm, based on the reaction quotient (Q) which direction would the reaction
proceed to reach equilibrium? (left or right)

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