1 (a) N2(g) O2(g) ZNO (g) AH298 = + 180 kJ mol-! From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (b) Increasing the pressure (c) Increasing the temperature (d) Increasing the concentration of N2 (e) Adding a catalyst

1 (a) N2(g) O2(g) ZNO (g) AH298 = + 180 kJ mol-! From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (b) Increasing the pressure (c) Increasing the temperature (d) Increasing the concentration of N2 (e) Adding a catalyst

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 82QAP: A student studies the equilibrium I2(g)2I(g)at a high temperature. She finds that the total pressure...

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