As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseousmixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C.4 (g)Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products,or more reactants?N2O44 (9) → 2NO2 (9)Ko = 4.61 x 103 at 25°C

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As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (a) and 0.750 mol N204 (g) at 25°C. Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N204 (g) → 2NO2 (g) K = 4.61 x 10-3 at 25°C

As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (a) and 0.750 mol N204 (g) at 25°C. Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N204 (g) → 2NO2 (g) K = 4.61 x 10-3 at 25°C

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 32QAP: Consider the following reaction at 75C: 3R(s)+2Q(g)A(g)+5B(l)K=9.4 A 10.0-L sample contains 0.30 mol...

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