The Haber process is an equilibrium used to manufacture ammonia gas from nitrogen gas and hydrogen gas. The forward reaction is endothermic. Heat + 2NH3 (g) <=> 3H2 (g) + N2 (g) If the temperature of the reaction increases, a. Which direction does the equilibrium shift (right, left, no shift)? b. What happens to the concentration of the product N2 (increases, decreases, remains the same)? If the concentration of NH3 is decreased, c. Which direction does the equilibrium shift (right, left, no shift)? d. What happens to the concentration of product N2 (increases, decreases, remains the same)?
The Haber process is an equilibrium used to manufacture ammonia gas from nitrogen gas and hydrogen gas. The forward reaction is endothermic. Heat + 2NH3 (g) <=> 3H2 (g) + N2 (g) If the temperature of the reaction increases, a. Which direction does the equilibrium shift (right, left, no shift)? b. What happens to the concentration of the product N2 (increases, decreases, remains the same)? If the concentration of NH3 is decreased, c. Which direction does the equilibrium shift (right, left, no shift)? d. What happens to the concentration of product N2 (increases, decreases, remains the same)?
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.100PAE: 12.100 A reaction important in smog formation is O3(g)+NO(g)O2(g)+NO2(g)K=6.01034 (a) If the initial...
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