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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.

Respuesta :

sebassandin

Answer:

[tex]K=4.07x10^{-4}[/tex]

Explanation:

Hello!

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

[tex]K=\frac{[CO]^4}{[Ni(CO)_4]}[/tex]

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

[tex][CO]_{EQ}=\frac{1.98g}{28.01g/mol} *\frac{1}{2.6L}=0.0272M[/tex]

[tex][Ni(CO)_4]_{EQ}=\frac{0.597g}{170.73g/mol} *\frac{1}{2.6L}=0.001345M[/tex]

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

[tex]K=\frac{(0.0272)^4}{[(0.001345)}\\\\K=4.07x10^{-4}[/tex]

Best regards!

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