Consider the following equilibrium process at 686°C:CO2(g) + H2(g) = CO(g) + H20(g)The equilibrium concentrations of the reacting species are [CO] = 0.0530 M, (H2] = 0.0440 M,[CO2]= 0.0880 M, and [H2O] = 0.0440 M.(a) Calculate K. for the reaction at 686°C.(b) If we add CO2 to increase its concentration to 0.520 mol / L, what will the concentrations of all thegases be when equilibrium is reestablished?Co:MH2:MCO:MH2O:M

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Consider the following equilibrium process at 686°C: CO2(g) + H2(g)= CO(g) + H20(g) 1l The equilibrium concentrations of the reacting species are [CO] = 0.0530 M, [H2] = 0.0440 M, [CO2] = 0.0880 M, and [H20] = 0.0440 M. %3D (a) Calculate K. for the reaction at 686°C. (b) If we add CO, to increase its concentration to 0.520 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M H2: CO: H,O: M

Consider the following equilibrium process at 686°C: CO2(g) + H2(g)= CO(g) + H20(g) 1l The equilibrium concentrations of the reacting species are [CO] = 0.0530 M, [H2] = 0.0440 M, [CO2] = 0.0880 M, and [H20] = 0.0440 M. %3D (a) Calculate K. for the reaction at 686°C. (b) If we add CO, to increase its concentration to 0.520 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M H2: CO: H,O: M

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter16: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 83AE: Consider the following system at equilibrium at 25C: PCl3(g)+Cl(g)PCl5(g)G=92.50KJ What will happen...

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