Consider the following equilibrium process between dinitrogen tetrafluoride and nitrogen difluoride. N2F4 (g) 2 NF2 (g) AH° = - 38.5 kJ/mol By expanding the expression for Kp for this reaction explain precisely what happens to the position of equilibrium when (i) the total pressure is increased, (ii) partial pressure of N2F4 is decreased.
Consider the following equilibrium process between dinitrogen tetrafluoride and nitrogen difluoride. N2F4 (g) 2 NF2 (g) AH° = - 38.5 kJ/mol By expanding the expression for Kp for this reaction explain precisely what happens to the position of equilibrium when (i) the total pressure is increased, (ii) partial pressure of N2F4 is decreased.
Chemistry for Engineering Students
3rd Edition
ISBN:9781285199023
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.27PAE
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