[Sis290025]

A mixture of 0.223 mol CO2, 0.230 mol of H2, and 0.343 mol of H2O are placed in a 2.0 L container. The following equilibrium is established: CO2 + H2 <-> CO + H2O. The equilibrium concentration of H2O is 0.210 M. Calculate the equilibrium constant (Kc).


Well, K_c = [CO][H2O]/[CO2][H2]

H20, I am assuming, is a gas.

---------------------CO2-----------H2-----------CO-------------H2O
Initial M-----------0.1115--------0.1150-------0---------------0.1715
delta M_________negative x_____neg x________(+x)_________(+x)
Equilibrium M____________________________________________0.210

M_i CO2 = 0.223 mol/2.0 L = 0.1115 M
M_i H2 = 0.230 mol/2.0 L =0.1150 M
M_i H20 = 0.343 mol/2.0 L = 0.1715  M


Now change or x = 0.210 M - 0.1715 M = 0.0385 M?

So

[CO] = 0 + x = 0.0385 M
[H20] = 0.210 M

[CO2] = 0.1115 - x = 0.1115 - 0.0385
[H2] =0.1150 - x = 0.1150 - 0.0385

K_c =  [0.0385][0.210]/[0.1115-0.0385 ][1150 - 0.0385] = 1.45  



Please help. Thanks.