(b), Ammonia is made from N; and H: by the following reversible reactions: N:(g) + 3H:(g) 2NH>(g) Assume that the initial concentrations of both N2 and H2 are 0.100 mol/L. Calculate the equilibrium concentrations of the three components of this reaction at 500°C if the equilibrium constant for the reaction at the temperature is 0.040. Assume further that the amount ofN: used is so small that subtracting it from 0.0100 mol/L or even subtracting it from three times H, does not make a significant change from the initial concentrations of N, and H.

(b), Ammonia is made from N; and H: by the following reversible reactions: N:(g) + 3H:(g) 2NH>(g) Assume that the initial concentrations of both N2 and H2 are 0.100 mol/L. Calculate the equilibrium concentrations of the three components of this reaction at 500°C if the equilibrium constant for the reaction at the temperature is 0.040. Assume further that the amount ofN: used is so small that subtracting it from 0.0100 mol/L or even subtracting it from three times H, does not make a significant change from the initial concentrations of N, and H.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.18PAE: The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures...

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