Given that the following reversible reaction: 2NH3(g) ⇌ N2(g) +3H2(g) ; If 0.64 mols of NH3 is added to an empty 750 mL container and allowed to reach equilibrium at which point the concentration of NH3 = 0.15M, predict the equilibrium concentrations of N2 (g) and H2 (g) answer should follow the format: a) Initial Molarity of (i) NH3(g) (ii) N2(g) (iii) H2(g) b) Change (using + or - x values) (i) NH3(g) (ii) N2(g) (iii) H2(g) c) the value of X d) Equilibrium Molarity of (i) NH3(g) (ii) N2(g) (iii) H2(g)
Given that the following reversible reaction: 2NH3(g) ⇌ N2(g) +3H2(g) ; If 0.64 mols of NH3 is added to an empty 750 mL container and allowed to reach equilibrium at which point the concentration of NH3 = 0.15M, predict the equilibrium concentrations of N2 (g) and H2 (g) answer should follow the format: a) Initial Molarity of (i) NH3(g) (ii) N2(g) (iii) H2(g) b) Change (using + or - x values) (i) NH3(g) (ii) N2(g) (iii) H2(g) c) the value of X d) Equilibrium Molarity of (i) NH3(g) (ii) N2(g) (iii) H2(g)
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
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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Given that the following reversible reaction: 2NH3(g) ⇌ N2(g) +3H2(g) ;
If 0.64 mols of NH3 is added to an empty 750 mL container and allowed to reach equilibrium at which point the concentration of NH3 = 0.15M, predict the equilibrium concentrations of N2 (g) and H2 (g)
answer should follow the format:
a) Initial Molarity of (i) NH3(g) (ii) N2(g) (iii) H2(g)
b) Change (using + or - x values) (i) NH3(g) (ii) N2(g) (iii) H2(g)
c) the value of X
d) Equilibrium Molarity of (i) NH3(g) (ii) N2(g) (iii) H2(g)
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