[staticbubblegum]

so confused by these and would really appreciate some help

1. solid ammonium carbamate, NH4CO2NH2, decomposes into ammonia gas and carbon dioxide. Calculate the value of the equilibrium constant for this system at 40*C if the combined gas concentration is 1.41 x 10^-2 mol/L

this is what i have so far for the ice table
NH4CO2NH2 (s) --> 2NH3 (g) + CO2 (g)
I          -               0                    0
C         -               +2x               +x
E         -        0.0094mol/l   0.0047mol/l
I was wondering if because the combined concentration is 1.41 x 10^-2 do you have to spread it across NH3 and CO2 so the equilibrium concentrations are 0.0094mol/l (because coefficient of 2) and 0.0047??

{Mod Edit: Removed the yelling -- STOP SCROLLING! }

[Borek]

Please don't cross post.

You have to show your attempts at solving the question to receive help. This is a forum policy.

[staticbubblegum]

sorry guys I'm new to the site! I reposted with some of the work I've done would be good to know if I'm on the right track

[Borek]

I was wondering if because the combined concentration is 1.41 x 10^-2 do you have to spread it across NH3 and CO2 so the equilibrium concentrations are 0.0094mol/l (because coefficient of 2) and 0.0047??

Yes, that's a correct approach.