1- The following equilibrium pressures were observed at a certain temperature for the reaction N2 (g)+ 3H2 (g)-→2NH3(g) PNH3 = 3.1 × 10² atm, Pn2 = 8.5 × 10' atm, and PH2 = 3.1 × 10³ atm Calculate the value for the equilibrium constant Kp at this temperature. If Py2 = 0.525 atm, PNH3 = 0.0167 atm, and PH2 = 0.00761 atm, does this represent a system at equilibrium?
1- The following equilibrium pressures were observed at a certain temperature for the reaction N2 (g)+ 3H2 (g)-→2NH3(g) PNH3 = 3.1 × 10² atm, Pn2 = 8.5 × 10' atm, and PH2 = 3.1 × 10³ atm Calculate the value for the equilibrium constant Kp at this temperature. If Py2 = 0.525 atm, PNH3 = 0.0167 atm, and PH2 = 0.00761 atm, does this represent a system at equilibrium?
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter13: Fundamental Equilibrium Concepts
Section: Chapter Questions
Problem 90E: In a 3.0-L vessel, the following equilibrium partial pressures are measured: N2, 190 torr; H2, 317...
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