CO(g)+2H2(g)⇌CH3OH(g)CO(g)+2H2(g)⇌C H3OH(g) This reaction is carried out at a different temperature with initial concentrations of [CO]=0.27M[CO]=0.27M and [H2]=0.49M[H2]=0.49M. At equilibrium, the concentration of CH3OHCH3OH is 0.11 MM. Find the equilibrium constant at this temperature.

9.4

Explanation:

The equation for the reaction can be represented as:

   +         ⇄  

The ICE table can be represented as:

                                     +         ⇄  

Initial                          0.27             0.49              0.0

Change                      -x                  -2x                 x

Equilibrium               0.27 - x         0.49 -2x          x

We can now say that the concentration of   at equilibrium is x;

Let's not forget that at equilibrium   = 0.11 M

So:

x =  [] = 0.11 M

[] = 0.27 - x

[] = 0.27 - 0.11

[] = 0.16 M

[] = (0.49 - 2x)

[] = (0.49 - 2(0.11))

[] = 0.49 - 0.22

[] = 0.27 M

= 9.4

∴ The equilibrium constant at that temperature = 9.4

the answer is 303.15 or 303