Asked by Katie
Consider this reaction: CO (g) + H2O (g0 <---> CO2(g)+H2(g)
kc=102 at 500 K
A reaction mixture initially contains 0.145 M of CO and 0.145 M of H20. What would be the equilibrium concentration of [CO]?
I so far have
kc= [H2][CO2]/[CO][H2O]= 102
I know i have to set up an ice table so i have:
CO H2O CO2 H2
I 0.145 M 0.145M 0 0
C -x -x +x +x
E
what do i do now? i'm kind of stuck. thank you!
kc=102 at 500 K
A reaction mixture initially contains 0.145 M of CO and 0.145 M of H20. What would be the equilibrium concentration of [CO]?
I so far have
kc= [H2][CO2]/[CO][H2O]= 102
I know i have to set up an ice table so i have:
CO H2O CO2 H2
I 0.145 M 0.145M 0 0
C -x -x +x +x
E
what do i do now? i'm kind of stuck. thank you!
Answers
Answered by
DrBob222
Add the columns so that initial column + change column = equilibrium column.
Equilibrium:
CO = 0.145-x
H2O = 0.145-x
CO2 = x
H2 = x
Now substitute those values into your Kc expression and solve for x.
Equilibrium:
CO = 0.145-x
H2O = 0.145-x
CO2 = x
H2 = x
Now substitute those values into your Kc expression and solve for x.