Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron mesh impregnated with oxides as a catalyst. For the reaction N2 (g) + H2 (g) NH3 (g) equilibrium constants (Kp values) as a function of temperature are 300 °C 4.34E-3 500 °C 2.25E-6 ln(?2?1)=−∆??(1?2−1?1) a) Is the reaction exothermic or endothermic? b) Using equilibrium principles explain what would happen to K if the reaction was opposite of what you found in the first part and the temperature decreased
Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron mesh impregnated with oxides as a catalyst. For the reaction N2 (g) + H2 (g) NH3 (g) equilibrium constants (Kp values) as a function of temperature are 300 °C 4.34E-3 500 °C 2.25E-6 ln(?2?1)=−∆??(1?2−1?1) a) Is the reaction exothermic or endothermic? b) Using equilibrium principles explain what would happen to K if the reaction was opposite of what you found in the first part and the temperature decreased
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
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 80E: Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using...
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Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron mesh impregnated with oxides as a catalyst. For the reaction
N2 (g) + H2 (g) NH3 (g)
equilibrium constants (Kp values) as a function of temperature are
300 °C 4.34E-3
500 °C 2.25E-6
ln(?2?1)=−∆??(1?2−1?1)
a) Is the reaction exothermic or endothermic?
b) Using equilibrium principles explain what would happen to K if the reaction was opposite of what you found in the first part and the temperature decreased
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