(d) The analysis of gases in a sealed reaction vessel containing NH3, N2, and H2 at equilibrium at 400°C determined the Ke 0.50 No(g)+3H2(g) 2NH3 (g) i. Write the Ke and K, expressions for the reaction. ii. Calculate the K, value of the reaction at 400°C iii.If the initial N2 and H2 concentrations are 0.100 M and 0.240 M respectively, calculate the following: A. the equilibrium concentrations of both the reactants and products; B. the percentage of unreacted reactant concentrations at equilibrium.

Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
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Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 36QAP: At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s),...
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Questions d(a) and d(b). I have completed other parts. 

(d) The analysis of gases in a sealed reaction vessel containing NH3, N2, and H2 at equilibrium at
400°C determined the Ke 0.50
No(g)+3H2(g) 2NH3 (g)
i. Write the Ke and K, expressions for the reaction.
ii. Calculate the K, value of the reaction at 400°C
iii.If the initial N2 and H2 concentrations are 0.100 M and 0.240 M respectively, calculate the
following:
A. the equilibrium concentrations of both the reactants and products;
B. the percentage of unreacted reactant concentrations at equilibrium.
Transcribed Image Text:(d) The analysis of gases in a sealed reaction vessel containing NH3, N2, and H2 at equilibrium at 400°C determined the Ke 0.50 No(g)+3H2(g) 2NH3 (g) i. Write the Ke and K, expressions for the reaction. ii. Calculate the K, value of the reaction at 400°C iii.If the initial N2 and H2 concentrations are 0.100 M and 0.240 M respectively, calculate the following: A. the equilibrium concentrations of both the reactants and products; B. the percentage of unreacted reactant concentrations at equilibrium.
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