QUESTION 13Consider the following reaction and its equilibrium constant at 100°C: N2O4(g) ⇌ 2NO2(g) Keq = 6.5If 0.250 mol of each reactant and product is mixed into a 2.0−L container, will the reaction proceed in the forward or reverse direction, or is it already at equilibrium? Since Q = 8, the reaction will proceed in the forward direction because there is too much NO2 and too little N2O4 in the system. The reaction is already at equilibrium. Since Q = 0.125, the reaction will proceed in the forward direction because there is too much N2O4 and too little NO2 in the system. Since Q = 8, the reaction will proceed in the reverse direction because there is too much NO2 and too little N2O4 in the system. Since Q = 0.125, the reaction will proceed in the reverse direction because there is too much N2O4 and too little NO2 in the system.

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Answered: Consider the following reaction and its…

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

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QUESTION 13

Consider the following reaction and its equilibrium constant at 100°C:

N₂O₄(g) ⇌ 2NO₂(g)

K_eq = 6.5

If 0.250 mol of each reactant and product is mixed into a 2.0−L container, will the reaction proceed in the forward or reverse direction, or is it already at equilibrium?

		Since Q = 8, the reaction will proceed in the forward direction because there is too much NO₂ and too little N₂O₄ in the system.
		The reaction is already at equilibrium.
		Since Q = 0.125, the reaction will proceed in the forward direction because there is too much N₂O₄ and too little NO₂ in the system.
		Since Q = 8, the reaction will proceed in the reverse direction because there is too much NO₂ and too little N₂O₄ in the system.
		Since Q = 0.125, the reaction will proceed in the reverse direction because there is too much N₂O₄ and too little NO₂ in the system.

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