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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 spe- cies are [CO] = 0.050 M, [H₂] = 0.045 M. [CO]= 0.086 M, and [H₂O] = 0.040 M. (a) Calculate K for the reaction at 686°C. (b) If we add CO₂ to increase its concentration to 0.50 mol/L, what will the con- centrations 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 spe- cies are [CO] = 0.050 M, [H₂] = 0.045 M. [CO]= 0.086 M, and [H₂O] = 0.040 M. (a) Calculate K for the reaction at 686°C. (b) If we add CO₂ to increase its concentration to 0.50 mol/L, what will the con- centrations of all the gases be when equilibrium is reestablished?

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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 spe- cies are [CO] = 0.050 M, [H₂] = 0.045 M. [CO₂] = 0.086 M, and [H₂O] = 0.040 M. (a) Calculate K, for the reaction at 686°C. (b) If we add CO₂ to increase its concentration to 0.50 mol/L, what will the con- centrations of all the gases be when equilibrium is reestablished?
Transcribed Image Text:Consider the following equilibrium process at 686°C: CO₂(g) + H₂(g) = CO(g) + H₂O(g) The equilibrium concentrations of the reacting spe- cies are [CO] = 0.050 M, [H₂] = 0.045 M. [CO₂] = 0.086 M, and [H₂O] = 0.040 M. (a) Calculate K, for the reaction at 686°C. (b) If we add CO₂ to increase its concentration to 0.50 mol/L, what will the con- centrations of all the gases be when equilibrium is reestablished?
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