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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)

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
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
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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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