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= atmPC6H5CHO= atmPH2= atmB.) 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 =

Given Kp, for the following reaction is 0.558 at 523 K: C6H5CH2OH(g) C6H5CHO(g) + H2(g) We have to…

Answered: The equilibrium constant, Kp, for the…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

A.) The equilibrium constant, K_p, 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.

P_C6H5CH2OH	=	atm
P_C6H5CHO	=	atm
P_H2	=	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, K_p, he obtained for this reaction.

K_p =