Consider the reaction: N2O4 (g) ⟷ 2 NO2 (g) KP = 0.36 (at 100°C) The reaction above is carried out at the same temperature but the vessel contains only the reactant, PN2O4 = 0.0550 atm and none of the product. Complete an ICE diagram to find the equilibrium partial pressures for N2O4 and NO2.
Consider the reaction: N2O4 (g) ⟷ 2 NO2 (g) KP = 0.36 (at 100°C) The reaction above is carried out at the same temperature but the vessel contains only the reactant, PN2O4 = 0.0550 atm and none of the product. Complete an ICE diagram to find the equilibrium partial pressures for N2O4 and NO2.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 72SCQ: Consider the formation of NO(g) from its elements. N2(g) + O2(g) 2 NO(g) (a) Calculate Kp at 25 C....
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Consider the reaction:
N2O4 (g) ⟷ 2 NO2 (g) KP = 0.36 (at 100°C)
The reaction above is carried out at the same temperature but the vessel contains only the reactant, PN2O4
= 0.0550
atm and none of the product. Complete an ICE diagram to find the equilibrium partial pressures for N2O4 and NO2.
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