1. A sample of ammonia gas was allowed to come to equilibrium at 400 K.2NH3(g)N2(g) + 3H2(g)At equilibrium, it was found that the concentration of H2 was 0.0551 M and theconcentration of N2 was 0.0183 M. If the Ke for this is 2.09 × 10-5, calculate the equilibriumconcentration of Ammonia.2 A sample of NX; gas was allowed to come to equilibrium at 400 K.2NX3(g) F N2(g) + 3X2(g)At equilibrium, it was found that the concentration of X2 was 0.078 M, and theconcentration of NX3 was 0.287 M. What was the initial concentration of NX3?

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A sample of ammonia gas was allowed to come to equilibrium at 400 K. 2NH3(g) N2(g) + 3H2(g) At equilibrium, it was found that the concentration of H2 was 0.0551 M and the concentration of N2 was 0.0183 M. If the Ke for this is 2.09 x 10-5, calculate the equilibrium concentration of Ammonia.

A sample of ammonia gas was allowed to come to equilibrium at 400 K. 2NH3(g) N2(g) + 3H2(g) At equilibrium, it was found that the concentration of H2 was 0.0551 M and the concentration of N2 was 0.0183 M. If the Ke for this is 2.09 x 10-5, calculate the equilibrium concentration of Ammonia.

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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1. A sample of ammonia gas was allowed to come to equilibrium at 400 K.
2NH3(g)
N2(g) + 3H2(g)
At equilibrium, it was found that the concentration of H2 was 0.0551 M and the
concentration of N2 was 0.0183 M. If the Ke for this is 2.09 × 10-5, calculate the equilibrium
concentration of Ammonia.
2 A sample of NX; gas was allowed to come to equilibrium at 400 K.
2NX3(g) F N2(g) + 3X2(g)
At equilibrium, it was found that the concentration of X2 was 0.078 M, and the
concentration of NX3 was 0.287 M. What was the initial concentration of NX3?

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