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] = 0.0500 M, [H2] = 0.0430 M, [CO2] = %3D = 0.0850 M, and [H,O] = 0.0350 M. (a) Calculate K, for the reaction at 686°C. (b) If we add CO, to increase its concentration to 0.430 mol / L, what will the concentrations of all gases be when equilibrium is reestablished? CO2: M H2: M CO: M H,O: M
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] = 0.0500 M, [H2] = 0.0430 M, [CO2] = %3D = 0.0850 M, and [H,O] = 0.0350 M. (a) Calculate K, for the reaction at 686°C. (b) If we add CO, to increase its concentration to 0.430 mol / L, what will the concentrations of all gases be when equilibrium is reestablished? CO2: M H2: M CO: M H,O: M
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![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] = 0.0500 M, [H2] = 0.0430 M,
[CO2] = 0.0850 M, and [H2O] = 0.0350 M.
%3D
(a) Calculate K, for the reaction at 686°C.
(b) If we add CO, to increase its concentration to 0.430 mol / L, what will the concentrations of all
gases be when equilibrium is reestablished?
CO2:
M
H2:
M
СО:
M
H,O:
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe677af44-8ce0-4cbe-83ef-37119dabbe6b%2F0b368935-9cbf-487c-9056-48c8313c671f%2Flxj9a8u_processed.png&w=3840&q=75)
Transcribed Image Text: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] = 0.0500 M, [H2] = 0.0430 M,
[CO2] = 0.0850 M, and [H2O] = 0.0350 M.
%3D
(a) Calculate K, for the reaction at 686°C.
(b) If we add CO, to increase its concentration to 0.430 mol / L, what will the concentrations of all
gases be when equilibrium is reestablished?
CO2:
M
H2:
M
СО:
M
H,O:
M
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