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For the reaction CuS(s) + H 2(g) H 2S(g) + Cu(s), AG° (CuS) = -53.6 kJ/mol AG (H 2S) = -33.6 kJ/mol AH° (CuS) = -53.1 kJ/mol AH° (H 2S) = - -20.6 kJ/mol Calculate the value of the equilibrium constant (K p) at 798 K and 1 atm pressure.

For the reaction CuS(s) + H 2(g) H 2S(g) + Cu(s), AG° (CuS) = -53.6 kJ/mol AG (H 2S) = -33.6 kJ/mol AH° (CuS) = -53.1 kJ/mol AH° (H 2S) = - -20.6 kJ/mol Calculate the value of the equilibrium constant (K p) at 798 K and 1 atm pressure.

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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For the reaction CuS(s) + H 2(g) H 2S(g) + Cu(s), AG° r (CuS) = -53.6 kJ/mol AG° (H 2S) -33.6 kJ/mol AH° t (CuS) = -53.1 kJ/mol AH° t (H 2S)=-20.6 kJ/mol %3D Calculate the value of the equilibrium constant (K p) at 798 K and 1 atm pressure. O 1.37 O 1.77 O 1.57 O 1.17 O None of the above
Transcribed Image Text:For the reaction CuS(s) + H 2(g) H 2S(g) + Cu(s), AG° r (CuS) = -53.6 kJ/mol AG° (H 2S) -33.6 kJ/mol AH° t (CuS) = -53.1 kJ/mol AH° t (H 2S)=-20.6 kJ/mol %3D Calculate the value of the equilibrium constant (K p) at 798 K and 1 atm pressure. O 1.37 O 1.77 O 1.57 O 1.17 O None of the above
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