Respuesta :
The question is incomplete, here is the complete question:
Nickel and carbon monoxide react to form nickel carbonyl, like this:
[tex]Ni(s)+4CO(g)\rightarrow Ni(CO)_4(g)[/tex]
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
[tex]Ni(CO)_4[/tex] 0.597 g
Calculate the value of the equilibrium constant.
Answer: The value of equilibrium constant for the reaction is 2448.1
Explanation:
We are given:
Mass of nickel = 12.7 g
Mass of CO = 1.98 g
Mass of [tex]Ni(CO)_4[/tex] = 0.597 g
Volume of container = 2.6 L
To calculate the number of moles for given molarity, we use the equation:
[tex]\text{Molarity of the solution}=\frac{\text{Given mass of solute}}{\text{Molar mass of solute}\times \text{Volume of solution (in L)}}[/tex]
[tex]\text{Equilibrium concentration of nickel}=\frac{12.7}{58.7\times 2.6}=0.083M[/tex]
[tex]\text{Equilibrium concentration of CO}=\frac{1.98}{28\times 2.6}=0.0272M[/tex]
[tex]\text{Equilibrium concentration of }Ni(CO)_4=\frac{0.597}{170.73\times 2.6}=0.00134M[/tex]
For the given chemical reaction:
[tex]Ni(s)+4CO(g)\rightarrow Ni(CO)_4(g)[/tex]
The expression of equilibrium constant for the reaction:
[tex]K_{eq}=\frac{[Ni(CO)_4]}{[CO]^4}[/tex]
Concentrations of pure solids and pure liquids are taken as 1 in equilibrium constant expression.
Putting values in above expression, we get:
[tex]K_{eq}=\frac{0.00134}{(0.0272)^4}\\\\K_{eq}=2448.1[/tex]
Hence, the value of equilibrium constant for the reaction is 2448.1
