The formation of nitrogen monoxide from its elements has an equilibrium which favors reactants: N2 (g) + O2 (g) → 2 NO (g) Kp = 0.0290 at 2400°C If the initial partial pressures of both reactant gases are 0.717 atm, what will be the equilibrium partial pressure of nitrogen monoxide? (A certain simplification is valid in solving this problem). (A) (B) (C) (D) (E) 0.112 atm 0.0290 atm 0.688 atm 0.0563 atm 0.0611 atm
The formation of nitrogen monoxide from its elements has an equilibrium which favors reactants: N2 (g) + O2 (g) → 2 NO (g) Kp = 0.0290 at 2400°C If the initial partial pressures of both reactant gases are 0.717 atm, what will be the equilibrium partial pressure of nitrogen monoxide? (A certain simplification is valid in solving this problem). (A) (B) (C) (D) (E) 0.112 atm 0.0290 atm 0.688 atm 0.0563 atm 0.0611 atm
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 34QAP: At 500C, k for the for the formation of ammonia from nitrogen and hydrogen gases is 1.5105....
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