Question

Nickel and carbon monoxide react to form nickel carbonyl, like this: (s)(g)(g) At a certain temperature, a chemist finds that a reaction vessel containing a mixture of nickel, carbon monoxide, and nickel carbonyl at equilibrium has the following composition: compound amount

Calculate the value of the equilibrium constant

Answer 1

The question is incomplete, here is the complete question:

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

`Ni(s)+4CO(g)\rightarrow Ni(CO)_4(g)`

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

`Ni(CO)_4` 0.597 g

Calculate the value of the equilibrium constant.

Answer: The value of equilibrium constant for the reaction is 2448.1

Step-by-step explanation:

We are given:

Mass of nickel = 12.7 g

Mass of CO = 1.98 g

Mass of
`Ni(CO)_4` = 0.597 g

Volume of container = 2.6 L

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

`\text{Molarity of the solution}=\frac{\text{Given mass of solute}}{\text{Molar mass of solute}* \text{Volume of solution (in L)}}`

`\text{Equilibrium concentration of nickel}=(12.7)/(58.7* 2.6)=0.083M`

`\text{Equilibrium concentration of CO}=(1.98)/(28* 2.6)=0.0272M`

`\text{Equilibrium concentration of }Ni(CO)_4=(0.597)/(170.73* 2.6)=0.00134M`

For the given chemical reaction:

`Ni(s)+4CO(g)\rightarrow Ni(CO)_4(g)`

The expression of equilibrium constant for the reaction:

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

Concentrations of pure solids and pure liquids are taken as 1 in equilibrium constant expression.

Putting values in above expression, we get:

`K_(eq)=(0.00134)/((0.0272)^4)\\\\K_(eq)=2448.1`

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