<u>Answer:</u> The moles of
added to the system is 7.13 moles
<u>Explanation:</u>
We are given:
Moles of
at equilibrium = 1.00 moles
Moles of
at equilibrium = 1.00 moles
Moles of
at equilibrium = 2.40 moles
Moles of
at equilibrium = 2.40 moles
Volume of the container = 4.00 L
Concentration is written as:

The given chemical equation follows:

The expression of
for above equation follows:
![K_c=\frac{[CO][H_2O]}{[CO_2][H_2]}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%5BCO%5D%5BH_2O%5D%7D%7B%5BCO_2%5D%5BH_2%5D%7D)
Putting values in above equation, we get:

To calculate the number of moles for given molarity, we use the equation:

Molarity of CO = 0.791 mol/L
Volume of solution = 4.00 L
Putting values in above equation, we get:

Extra moles of CO = (3.164 - 2.40) = 0.764 moles
Let the moles of
needed be 'x' moles.
Now, equilibrium gets re-established:

Initial: 1.00 1.00 2.40 2.40
At eqllm: (0.236+x) 0.236 3.164 3.164
Again, putting the values in the expression of
, we get:

Hence, the moles of
added to the system is 7.13 moles