The question is incomplete, here is the complete question:
Nickel and carbon monoxide react to form nickel carbonyl, like this:
At a certain temperature, a chemist finds that a 2.6 L reaction vessel containing a mixture of nickel, carbon monoxide, and nickel carbonyl at equilibrium has the following composition:
Compound Amount
Ni 12.7 g
CO 1.98 g
0.597 g
Calculate the value of the equilibrium constant.
<u>Answer:</u> The value of equilibrium constant for the reaction is 2448.1
<u>Explanation:</u>
We are given:
Mass of nickel = 12.7 g
Mass of CO = 1.98 g
Mass of
= 0.597 g
Volume of container = 2.6 L
To calculate the number of moles for given molarity, we use the equation:




For the given chemical reaction:

The expression of equilibrium constant for the reaction:
![K_{eq}=\frac{[Ni(CO)_4]}{[CO]^4}](https://tex.z-dn.net/?f=K_%7Beq%7D%3D%5Cfrac%7B%5BNi%28CO%29_4%5D%7D%7B%5BCO%5D%5E4%7D)
Concentrations of pure solids and pure liquids are taken as 1 in equilibrium constant expression.
Putting values in above expression, we get:

Hence, the value of equilibrium constant for the reaction is 2448.1