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] = 0.0540 M, (H) = 0.0400 M, [CO2] = 0.0830 M, and [H2O] = 0.0360 M. (a) Calculate K, for the reaction at 686°C. (b) If we add CO, to increase its concentration to 0.440 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M H2: CO: M H2O: M
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] = 0.0540 M, (H) = 0.0400 M, [CO2] = 0.0830 M, and [H2O] = 0.0360 M. (a) Calculate K, for the reaction at 686°C. (b) If we add CO, to increase its concentration to 0.440 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M H2: CO: M H2O: M
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 28P
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