[GengiMane]

I was giving a practice question from my chemistry teacher which has stumped me. I have the reaction CO+Br2=CoBr2. Where [COBr2] = 0.12M, [CO] = 0.060M, [Br2] = 0.080M. The equilibrium constant is 25, but how can I verify the equilibrium constant is the same when the volume is doubled and 0.010M of COBr2 turns in CO and Br2?

I've tried subtracting and adding 0.01M of COBr to CO and Br. But I still cannot get the equilibrium constant back 25.
Any help is greatly appreciated thanks.

[chenbeier]

Double of Volume means half of the Mole before equlibrium
 COBr₂ = 0,06 M, CO = 0,03 M and Br₂ = 0,04 M.
New equlibrium change 0.01 M means COBr₂ = 0,05 M CO = 0,04 M and Br₂ = 0,05 M

K = 0,05 M/(0,04. M * 0.05 M)  = 25 q.e.d.

[GengiMane]

Oml thank you so much I see where I went wrong. I was adding just 0.005M to CO and 0.005M Br2.