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Given that the following reversible reaction: 2NH3(2) If 0.64 mols of NH, 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) +3H2(8) ; %3D N2 (g) and H, (g) Your answer should follow the format: a) Initial Molarity of (1) 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(2) If 0.64 mols of NH, 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) +3H2(8) ; %3D N2 (g) and H, (g) Your answer should follow the format: a) Initial Molarity of (1) 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
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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Given that the following reversible reaction: 2NH3(9) - N2g) +3H2(g) ; If 0.64 mols of NH, 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 H, (g) Your 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)
Transcribed Image Text:Given that the following reversible reaction: 2NH3(9) - N2g) +3H2(g) ; If 0.64 mols of NH, 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 H, (g) Your 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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