Hello, I'm trying to solve this equilibrium question and it's frustrating me to no end:
Reaction: Ni(s) + 4CO(g) <--> Ni(CO4)(g) Kc=1.8x1011
The question is: Initially 0.010 mol/L of Ni(CO4) is placed in a closed container with solid nickel, no CO is present. Calculate the equilibrium concentrations of CO and Ni(CO4).
Here's the work I did:
4CO <---> Ni(CO4)
I 0.00 0.010
C +4x -x
E +4x 0.010 - x
Then:
Kc = (0.010-x)/(4x)4=1.8x1011
0.010 - x = (1.8x1011)(256x4)
0 = 4.61x1013x4 + x - 0.010
Can't put that into a quadratic, so I guess I have to use a simplifying assumption and/or successive approximation, but I'm a bit confused as to how to proceed with that.
Any help would be greatly appreciated!
Regards,
M