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8) The following reaction is carried out at constant temperature and pressure. Use the given data for the reaction to answer parts a) through e). Assume that the reaction begins with 1 mole of P4(g). (50%) P4(g) 5 2P2(g) : AG:m = 225400 + 7.9TINT – 209.4T J a) Express the equilibrium constant (K) or reaction quotient (Q) in terms of the reaction extend (§). b) Calculate the extend of reaction when equilibrium is reached at 1300 K and 1 bar of total pressure.

8) The following reaction is carried out at constant temperature and pressure. Use the given data for the reaction to answer parts a) through e). Assume that the reaction begins with 1 mole of P4(g). (50%) P4(g) 5 2P2(g) : AG:m = 225400 + 7.9TINT – 209.4T J a) Express the equilibrium constant (K) or reaction quotient (Q) in terms of the reaction extend (§). b) Calculate the extend of reaction when equilibrium is reached at 1300 K and 1 bar of total 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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8) The following reaction is carried out at constant temperature and pressure. Use the given data for the reaction to answer parts a) through e). Assume that the reaction begins with 1 mole of P4(g). (50%) P4(g) 5 2P2(g) AGgxn = 225400 + 7.9TlnT – 209.4T J a) Express the equilibrium constant (K) or reaction quotient (Q) in terms of the reaction extend (}). b) Calculate the extend of reaction when equilibrium is reached at 1300 K and 1 bar of total pressure. c) Calculate the Gibbs free energy change (AGRXN) at 1300 K and 1 bar for = 0.5. d) Determine in which direction the reaction will proceed in c) to reach equilibrium. e) Calculate the partial pressures of P4 and P2 in equilibrium at 1300 K and 10 bars of total pressure.
Transcribed Image Text:8) The following reaction is carried out at constant temperature and pressure. Use the given data for the reaction to answer parts a) through e). Assume that the reaction begins with 1 mole of P4(g). (50%) P4(g) 5 2P2(g) AGgxn = 225400 + 7.9TlnT – 209.4T J a) Express the equilibrium constant (K) or reaction quotient (Q) in terms of the reaction extend (}). b) Calculate the extend of reaction when equilibrium is reached at 1300 K and 1 bar of total pressure. c) Calculate the Gibbs free energy change (AGRXN) at 1300 K and 1 bar for = 0.5. d) Determine in which direction the reaction will proceed in c) to reach equilibrium. e) Calculate the partial pressures of P4 and P2 in equilibrium at 1300 K and 10 bars of total pressure.
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