(V) In the following reaction, which of the statements is true, given the concentrations of each species? N2(g) + 3H2 = 2NH3(g), K = 9.60 [N2] = [H2] = 0.200M and [N H3] = 0.352M O The reaction is at equilibrium. equilibrium. O More nitrogen must be consumed to achieve equilibrium. cannot be established in the system. O More ammonia must form to achieve O More nitrogen and hydrogen must form to achieve equilibrium. O Equilibrium
(V) In the following reaction, which of the statements is true, given the concentrations of each species? N2(g) + 3H2 = 2NH3(g), K = 9.60 [N2] = [H2] = 0.200M and [N H3] = 0.352M O The reaction is at equilibrium. equilibrium. O More nitrogen must be consumed to achieve equilibrium. cannot be established in the system. O More ammonia must form to achieve O More nitrogen and hydrogen must form to achieve equilibrium. O Equilibrium
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 28QAP: For the system PCl5(g)PCl3(g)+Cl2(g)K is 26 at 300C. In a 1.0-L flask at 300C, a gaseous mixture...
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I don't understand this concenpt.
I know Q= 77.44 and K=9.60,
Q > K which means reactants are already favored, so why is the answer
"more nitrogen and hydrogen must form to achieve equilibrium" if the reactants are already favored?
are we trying to make the value of Q closer to 9.60 or are we trying to make the value of K closer to 77.44?
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