Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0480 M, [H2] = 0.0400 M, [CO2] = 0.0830 M, and [H2O] = 0.0420 M. (a) Calculate Kc for the reaction at 686°C. (b) If we add CO2 to increase its concentration to 0.480 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished?
Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0480 M, [H2] = 0.0400 M, [CO2] = 0.0830 M, and [H2O] = 0.0420 M. (a) Calculate Kc for the reaction at 686°C. (b) If we add CO2 to increase its concentration to 0.480 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished?
Introductory Chemistry: A Foundation
8th Edition
ISBN:9781285199030
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 20QAP
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Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g)
The equilibrium concentrations of the reacting species are [CO] = 0.0480 M, [H2] = 0.0400 M, [CO2] = 0.0830 M,
and [H2O] = 0.0420 M.(a) Calculate Kc for the reaction at 686°C. (b) If we add CO2 to increase its concentration to 0.480 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M
H2: M
CO: M
H2O: |
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