Consider the reaction N2(g)+O2(g)↽−−⇀2NO(g)N2(g)+O2(g)↽−−⇀2NO(g) that has an equilibrium constant, ?cKc, fof 4.10×10−44.10×10−4 at 17001700 °C. What percentage of O2O2 will react to form NO if 0.5430.543 mol N2N2 and 0.5430.543 mol O2O2 are added to a 0.8750.875 L container and allowed to come to equilbrium at 17001700 °C?
Consider the reaction N2(g)+O2(g)↽−−⇀2NO(g)N2(g)+O2(g)↽−−⇀2NO(g) that has an equilibrium constant, ?cKc, fof 4.10×10−44.10×10−4 at 17001700 °C. What percentage of O2O2 will react to form NO if 0.5430.543 mol N2N2 and 0.5430.543 mol O2O2 are added to a 0.8750.875 L container and allowed to come to equilbrium at 17001700 °C?
Physical Chemistry
2nd Edition
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Ball, David W. (david Warren), BAER, Tomas
Chapter5: Introduction To Chemical Equilibrium
Section: Chapter Questions
Problem 5.19E: 5.19. Assume that a reaction exists such that equilibrium occurs when the partial pressures of the...
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Consider the reaction
N2(g)+O2(g)↽−−⇀2NO(g)N2(g)+O2(g)↽−−⇀2NO(g)
that has an equilibrium constant, ?cKc, fof 4.10×10−44.10×10−4 at 17001700 °C. What percentage of O2O2 will react to form NO if 0.5430.543 mol N2N2 and 0.5430.543 mol O2O2 are added to a 0.8750.875 L container and allowed to come to equilbrium at 17001700 °C?
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