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At 35°C, K=1.6x10−5 for the reaction 2NOCl(g)↔2NO(g) + Cl2(g) a. Calculate the concentration of all species at equilibrium when 2.0 moles pure NOCl in a 2.0 L flask b. Calculate the equilibrium concentrations of all species when 1.0 mole of NOCl is mixed with 1.0 mole NO in a 1.0 L flask c. Calculate the equilibrium concentrations of all species 2.0 moles of NOCl is mixed with 1.0 mole of Cl2 in a 1.0 L flask

At 35°C, K=1.6x10−5 for the reaction 2NOCl(g)↔2NO(g) + Cl2(g) a. Calculate the concentration of all species at equilibrium when 2.0 moles pure NOCl in a 2.0 L flask b. Calculate the equilibrium concentrations of all species when 1.0 mole of NOCl is mixed with 1.0 mole NO in a 1.0 L flask c. Calculate the equilibrium concentrations of all species 2.0 moles of NOCl is mixed with 1.0 mole of Cl2 in a 1.0 L flask

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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At 35°C, K=1.6x10−5 for the reaction 2NOCl(g)↔2NO(g) + Cl2(g)
a. Calculate the concentration of all species at equilibrium when
2.0 moles pure NOCl in a 2.0 L flask
b. Calculate the equilibrium concentrations of all species when 1.0 mole of NOCl is mixed with 1.0 mole NO in a 1.0 L flask
c. Calculate the equilibrium concentrations of all species 2.0 moles of NOCl is mixed with 1.0 mole of Cl2 in a 1.0 L flask.

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