The reaction: 2NO2(g) ⇌ N2O4(g) is an exothermic reaction, ΔH=-58.0 kJ/molrxn at 0°C the KP is 58. If the initial partial pressures of both NO2(g) and N2O4(g) are 2.00 atm: A) Is the reaction at equilibrium? If not, what is the value of Q? B) Which direction will the reaction go to reach equilibrium? C) Use an ICE table to find the equilibrium pressures.
The reaction: 2NO2(g) ⇌ N2O4(g) is an exothermic reaction, ΔH=-58.0 kJ/molrxn at 0°C the KP is 58. If the initial partial pressures of both NO2(g) and N2O4(g) are 2.00 atm: A) Is the reaction at equilibrium? If not, what is the value of Q? B) Which direction will the reaction go to reach equilibrium? C) Use an ICE table to find the equilibrium pressures.
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 20QAP: Consider the following hypothetical reactions and their equilibrium constants at 75C,...
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3) The reaction: 2NO2(g) ⇌ N2O4(g) is an exothermic reaction, ΔH=-58.0 kJ/molrxn at 0°C the KP is 58. If the initial partial pressures of both NO2(g) and N2O4(g) are 2.00 atm: A) Is the reaction at equilibrium? If not, what is the value of Q? B) Which direction will the reaction go to reach equilibrium? C) Use an ICE table to find the equilibrium pressures.
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