Consider the equilibrium system described by the chemical reaction below. When 1.50 mol of CO2 and an 10.0 mol solid carbon are heated in a 20.0 L container at 1100 K, the equilibrium concentration of CO is 0.0700 M. Determine the concentrations of all species at equilibrium and then calculate the value of Kc for this reaction. C(s) + CO:(g) = 2 CO(g)
Consider the equilibrium system described by the chemical reaction below. When 1.50 mol of CO2 and an 10.0 mol solid carbon are heated in a 20.0 L container at 1100 K, the equilibrium concentration of CO is 0.0700 M. Determine the concentrations of all species at equilibrium and then calculate the value of Kc for this reaction. C(s) + CO:(g) = 2 CO(g)
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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Transcribed Image Text:Question 27 of 35
Consider the equilibrium system described by the chemical reaction below. When 1.50
mol of CO2 and an 10.0 mol solid carbon are heated in a 20.0 L container at 1100 K,
the equilibrium concentration of CO is 0.0700 M. Determine the concentrations of all
species at equilibrium and then calculate the value of Kc for this reaction.
C(s) + CO:(g) = 2 CO(g)
1
2
NEXT
へ
Based on the given values, fill in the ICE table to determine concentrations of all reactants and
products.
C(s)
CO:(g)
2 CO(g)
Initial (M)
10.0
1.50
Change (M)
Equilibrium (M)
RESET
1.50
10.0
20.0
0.500
0.150
0.0750
-0.0350
0.110
0.0400
0.0700
-0.0700
0.140
-0.140
0.0350
0.0050
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