Question

Nickel carbonyl decomposes to form nickel and carbon monoxide, like this:

Ni(CO)4(g) → Ni(s)+ 4CO(g)

At a certain temperature, a chemist finds that a 2.6 L reaction vessel containing a mixture of nickel carbonyl, nickel, and carbon monoxide at equilibrium has the following composition:

compound amount
Ni(CO)4 0.597g
Ni 12.7g
CO 1.98g

Required:
Calculate the value of the equilibrium constant for this reaction.

Answer 1

`K=4.07x10^(-4)`

Step-by-step explanation:

Hello!

In this case, according to the given chemical reaction, it is possible to set up the equilibrium expression as shown below:

`K=([CO]^4)/([Ni(CO)_4])`

Since the nickel product is solid and is not included. It means that the concentrations at equilibrium of CO and Ni(CO)₄ are:

`[CO]_(EQ)=(1.98g)/(28.01g/mol) *(1)/(2.6L)=0.0272M`

`[Ni(CO)_4]_(EQ)=(0.597g)/(170.73g/mol) *(1)/(2.6L)=0.001345M`

Thus, there equilibrium constant for the reaction turns out to be:

`K=((0.0272)^4)/([(0.001345))\\\\K=4.07x10^(-4)`

Best regards!