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The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K. NH,HS(s) =NH3(g)+ H,S(g) Calculate the equilibrium concentration of H,S when 0.474 moles of NH,HS(s) are introduced into a 1.00 L vessel at 298 K. [H,S] = M

The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K. NH,HS(s) =NH3(g)+ H,S(g) Calculate the equilibrium concentration of H,S when 0.474 moles of NH,HS(s) are introduced into a 1.00 L vessel at 298 K. [H,S] = M

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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The equilibrium constant, Ke, for the following reaction is 1.80×104 at 298 K. NH,HS(s): =NH3(g)+ H,S(g) Calculate the equilibrium concentration of H,S when 0.474 moles of NH,HS(s) are introduced into a 1.00 L vessel at 298 K. [H,S] = M
Transcribed Image Text:The equilibrium constant, Ke, for the following reaction is 1.80×104 at 298 K. NH,HS(s): =NH3(g)+ H,S(g) Calculate the equilibrium concentration of H,S when 0.474 moles of NH,HS(s) are introduced into a 1.00 L vessel at 298 K. [H,S] = M
The equilibrium constant, K., for the following reaction is 10.5 at 350 K. 2CH,Cl,(g) CH4(g) + CC14(g) Calculate the equilibrium concentrations of reactant and products when 0.283 moles of CH,Cl, are introduced into a 1.00 L vessel at 350 K. [CH,Cl,] = M [CH4] M [CC4] M
Transcribed Image Text:The equilibrium constant, K., for the following reaction is 10.5 at 350 K. 2CH,Cl,(g) CH4(g) + CC14(g) Calculate the equilibrium concentrations of reactant and products when 0.283 moles of CH,Cl, are introduced into a 1.00 L vessel at 350 K. [CH,Cl,] = M [CH4] M [CC4] M
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