Answer : The value of 
of the reaction is 10.5 and the reaction is product favored.
Explanation : Given,
Moles of 
at equilibrium = 0.0406 mole
Moles of 
at equilibrium = 0.170 mole
Moles of 
at equilibrium = 0.302 mole
Volume of solution = 2.00 L
First we have to calculate the concentration of 
at equilibrium.
Now we have to calculate the value of equilibrium constant.
The balanced equilibrium reaction is,
The expression of equilibrium constant for the reaction will be:
![K_c=\frac{[CH_3OH]}{[CO][H_2]^2}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%5BCH_3OH%5D%7D%7B%5BCO%5D%5BH_2%5D%5E2%7D)
Now put all the values in this expression, we get :
Therefore, the value of of the reaction is, 10.5
There are 3 conditions:
When 
; the reaction is product favored.
When 
; the reaction is reactant favored.
When 
; the reaction is in equilibrium.
As the value of . So, the reaction is product favored.
