The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K: NHẠHS(s) NH3(9) + H2S(g) Calculate the equilibrium partial pressure of H2S when 0.405 moles of NHAHS(s) is introduced into a 1.00 L vessel at 298 K. PH,s atm

The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K: NHẠHS(s) NH3(9) + H2S(g) Calculate the equilibrium partial pressure of H2S when 0.405 moles of NHAHS(s) is introduced into a 1.00 L vessel at 298 K. PH,s atm

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

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Question

Solve both please ASAP

The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K:
NH4HS(s) NH3(9) + H2S(g)
Calculate the equilibrium partial pressure of H2S when 0.405 moles of NHAHS(s) is introduced into a 1.00 L vessel at
298 K.
PH25
atm

The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K:
Co(g) + Cl2(g) =coCI2(9)
Calculate the equilibrium partial pressures of all species when CO and Cl2, each at an intitial partial pressure of 1.15
atm, are introduced into an evacuated vessel at 60 K.
Pco
atm
Pciz
atm
%3D
Pcociz
atm

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