The equilibrium constant, Kp, for the following reaction is 0.558 at 523 K: C6H5CH2OH(g) C6H5CHO(g) + H2(g) Calculate the equilibrium partial pressures of all species when C6H5CH2OH(g) is introduced
The equilibrium constant, Kp, for the following reaction is 0.558 at 523 K: C6H5CH2OH(g) C6H5CHO(g) + H2(g) Calculate the equilibrium partial pressures of all species when C6H5CH2OH(g) is introduced
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 60QRT
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A.) The equilibrium constant, Kp, for the following reaction is 0.558 at 523 K:
C6H5CH2OH(g) C6H5CHO(g) + H2(g)
Calculate the equilibrium partial pressures of all species when C6H5CH2OH(g) is introduced into an evacuated flask at a pressure of 1.56 atm at 523 K.
PC6H5CH2OH | = | atm |
PC6H5CHO | = | atm |
PH2 | = | atm |
B.) A student ran the following reaction in the laboratory at 295 K: 2NOBr(g) 2NO(g) + Br2(g)
When he introduced NOBr(g) at a pressure of 0.426 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of Br2(g) to be 0.114 atm.
Calculate the equilibrium constant, Kp, he obtained for this reaction.
Kp =
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