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6. For the reaction 2 HI = H2g) + I2u3) Keg = 0.016 at 500°C (a) If 1.0 mole of HI is placed in a 2.0-/ container and allowed to come to equilibrium at 500°C, calculate the equilibrium concentrations of H,, I,, and HI. (b) If 0.35 mole of HI is placed in a 0.75-f container and allowed to come to equilibrium at 500°C, calculate the equilibrium concentrations of H,, I,, and HI.

6. For the reaction 2 HI = H2g) + I2u3) Keg = 0.016 at 500°C (a) If 1.0 mole of HI is placed in a 2.0-/ container and allowed to come to equilibrium at 500°C, calculate the equilibrium concentrations of H,, I,, and HI. (b) If 0.35 mole of HI is placed in a 0.75-f container and allowed to come to equilibrium at 500°C, calculate the equilibrium concentrations of H,, I,, and HI.

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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6. For the reaction 2 HI = H2) + I2) Keg = 0.016 at 500°C (a) If 1.0 mole of HI is placed in a 2.0-/ container and allowed to come to equilibrium at 500°C, calculate the equilibrium concentrations of H,, I,, and HI. (b) If 0.35 mole of HI is placed in a 0.75-f container and allowed to come to equilibrium at 500°C, calculate the equilibrium concentrations of H, I,, and HI.
Transcribed Image Text:6. For the reaction 2 HI = H2) + I2) Keg = 0.016 at 500°C (a) If 1.0 mole of HI is placed in a 2.0-/ container and allowed to come to equilibrium at 500°C, calculate the equilibrium concentrations of H,, I,, and HI. (b) If 0.35 mole of HI is placed in a 0.75-f container and allowed to come to equilibrium at 500°C, calculate the equilibrium concentrations of H, I,, and HI.
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