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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) + CO2(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) + CO2(g) =2 CO(g)

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.34PAE: 1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was...
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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) + CO2(g) =2 CO(g) 1 2 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. C(s) CO2(g) 2 CO(g) + Initial (M) Change (M) Equilibrium (M) RESET 1.50 10.0 20.0 0.500 0.150 0.0750 0.0700 -0.0700 0.140 -0.140 0.0350 -0.0350 0.110 0.0400 0.0050 1L
Transcribed Image Text: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) + CO2(g) =2 CO(g) 1 2 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. C(s) CO2(g) 2 CO(g) + Initial (M) Change (M) Equilibrium (M) RESET 1.50 10.0 20.0 0.500 0.150 0.0750 0.0700 -0.0700 0.140 -0.140 0.0350 -0.0350 0.110 0.0400 0.0050 1L
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) + CO2(g) 2 CO(g) PREV 1 2 Based on the set up of your ICE table, construct the expression for Kc and then evaluate it. Do not combine or simplify terms. Ko 5 RESET [1.50] [0.500] [0.150] [0.0750] [0.0700] [0.140] [0.0400] [0.0050] [1.50]? [0.500]? [0.150]? [0.0750]? [0.0700]? [0.140]? [0.0400]? [0.0050]? 1.75 0.571 0.123 8.16 II II
Transcribed Image Text: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) + CO2(g) 2 CO(g) PREV 1 2 Based on the set up of your ICE table, construct the expression for Kc and then evaluate it. Do not combine or simplify terms. Ko 5 RESET [1.50] [0.500] [0.150] [0.0750] [0.0700] [0.140] [0.0400] [0.0050] [1.50]? [0.500]? [0.150]? [0.0750]? [0.0700]? [0.140]? [0.0400]? [0.0050]? 1.75 0.571 0.123 8.16 II II
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