Activity 3: Le Chatelier's Principle The Haber Process for the manufacture of ammonia from nitrogen and hydrogen involves this reversible reaction: N2(g) + 3H2(g) 2 2NH3(g) AHºrm = 92.6 kJ/mol The AH value shows that the reaction is exothermic. a) What would be the effect on the position of equilibrium if you increased the pressure? Explain your answer using Le Chatelier's Principle. b) In order to get the maximum possible percentage of ammonia in the equilibrium mixture, would you choose to use a high or a low temperature? Explain your answer using Le Chatelier's Principle.

Activity 3: Le Chatelier's Principle The Haber Process for the manufacture of ammonia from nitrogen and hydrogen involves this reversible reaction: N2(g) + 3H2(g) 2 2NH3(g) AHºrm = 92.6 kJ/mol The AH value shows that the reaction is exothermic. a) What would be the effect on the position of equilibrium if you increased the pressure? Explain your answer using Le Chatelier's Principle. b) In order to get the maximum possible percentage of ammonia in the equilibrium mixture, would you choose to use a high or a low temperature? Explain your answer using Le Chatelier's Principle.

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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