The decomposition of ammonia at 400 °C is: 2 NH3(g) = N2(g) + 3 H2(g). If the partial pressure of NH3 at equilibrium is 1.6 x 10-3 atm and the partial pressures of N2 and H2 are each 0.25 atm at equilibrium, what is the value for Kc (not Kp!) at 400°C for the forward reaction? Enter your answer in decimal format with two decimal places.

The decomposition of ammonia at 400 °C is: 2 NH3(g) = N2(g) + 3 H2(g). If the partial pressure of NH3 at equilibrium is 1.6 x 10-3 atm and the partial pressures of N2 and H2 are each 0.25 atm at equilibrium, what is the value for Kc (not Kp!) at 400°C for the forward reaction? Enter your answer in decimal format with two decimal places.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 6RQ: Distinguish between the terms equilibrium constant and reaction quotient. When Q = K, what does this...

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