At 7877 °C the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(9) is Kp 0.735. If the initial pressure of NO is 0.00172 atm, what are the equilibrium partial pressures of NO, N₂, and O₂? P(NO)= p(N2)= p(0₂)
At 7877 °C the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(9) is Kp 0.735. If the initial pressure of NO is 0.00172 atm, what are the equilibrium partial pressures of NO, N₂, and O₂? P(NO)= p(N2)= p(0₂)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter14: Chemical Equilibirum
Section: Chapter Questions
Problem 14.98QP: The equilibrium constant Kc for the synthesis of methanol, CH3OH. CO(g)+2H2(g)CH3OH(g) is 4.3 at...
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