Consider the following reaction: NiO (s) + CO (g) Ni (s) + CO2 (g) Kc = 4.0 x 103 (at 1500 K). If a mixture of solid nickel (II) oxide and 0.10 M carbon monoxide is allowed to come to equilibrium at 1500 K, what will be the equilibrium concentration of carbon dioxide?

Question

Consider the following reaction: 
NiO (s) + CO (g) <--> Ni (s) + CO2 (g) 
Kc = 4.0 x 103 (at 1500 K). 
If a mixture of solid nickel (II) oxide and 0.10 M carbon monoxide is allowed to come to equilibrium at 1500 K, what will be the equilibrium concentration of carbon dioxide?

anonymous · Answer

Ok, so I know how to solve this problem now. But initially I thought to solve by:
[CO2] = Kc * [CO]. Then by looking at the answer i realized I needed to do an ICE table. By looking at the problem how should I have known I needed to make an ICE table is what I'm wondering?

jfraser · Answer

when the problem gives you starting conditions and asks for equilibrium concentrations, you need to do an ICE box