How do you calculate the equilibrium constant with the absorbance of a substance and the absorbance constant? When given the equation: $$\ce{Fe^3+_{(aq)} + SCN^-_{(aq)} &lt;=&gt; FeSCN^2+_{(aq)}}$$

How do you calculate the equilibrium constant when given the slope of the absorbance vs concentration graph ($\pu{4317 M-1}$) and the absorbance of $\ce{FeSCN^{2+}}$ (0.276)

The following information is also given: $2.000\ \mathrm{mL}$ of a $0.00200\  \mathrm{M}$ solution of $\mathrm{KSCN}$ with $5.00\ \mathrm{mL}$ of $0.00200\ \mathrm{M}$ solution of $\ce{Fe(NO3)3}$ and $3.00\ \mathrm{mL}$ of water is combined. 

So from this, I assumed that the concentrations of $\ce{SCN-}$ and $\ce{Fe^{3+}}$ are both $0.002\ \mathrm{M}$. 

I found the concentration of $\ce{FeSCN^2+_{(aq)}}$ to be $\pu{6.39e-5 M}$ using this equation:

$$\mathrm{Absorbance} = \mathrm{slope}\cdot \mathrm{conc.}$$

$$\mathrm{conc.} = \frac{\mathrm{Absorbance}}{\mathrm{slope}}$$

$$\mathrm{conc.} = \frac{0.276}{\pu{4317 M-1}}$$

$$\mathrm{conc.} = \pu{6.39e-5 M}$$

Using this value, I used the equation for the K constant of an equilibrium:

$$\mathrm{K} = \frac{[\ce{FeSCN^2+}]}{[\ce{Fe^3+}][\ce{SCN^-}]}$$

$$\mathrm{K} = \frac{\pu{6.39e-5}}{0.002^2}$$

$$\mathrm{K} = 15.975$$

This did not turn out to be the correct answer, but I'm not sure why. I suspect the concentrations for the two reactions are not correct since the volumes are also given.
I'm following the outline from the comment by user21398.

Initial concentrations after mixing

The volume of the mixture is $V_\text{mix} = \pu{10 mL}$. Using the dilution law, I get the following concentrations:

$$\ce{[Fe^3+]_\text{initial}} = \pu{2.00 mM} \cdot  \frac{\pu{5 mL}}{\pu{10 mL}} = \pu{1.00 mM}$$

$$\ce{[SCN-]_\text{initial}} = \pu{2.00 mM} \cdot  \frac{\pu{2 mL}}{\pu{10 mL}} = \pu{0.400 mM}$$

Equilibrium concentrations

The equilibrium concentration of the complex is already calculated, $\ce{[FeSCN^2+]_\text{equil}}=\pu{6.39e−5 M}.$

To get the equilibrium concentrations of the reactants, we have to consider that some reacted:

$$\ce{[Fe^3+]_\text{equil}} = \ce{[Fe^3+]_\text{initial}} - \ce{[FeSCN^2+]_\text{equil}} $$ $$ = \pu{1.00e-3 M} - \pu{6.39e−5 M} = \pu{0.94e-3 M}$$

And similar for thiocyanide:

$$\ce{[SCN-]_\text{equil}} =  \ce{[SCN-]_\text{initial}} - \ce{[FeSCN^2+]_\text{equil}} $$ $$ =\pu{0.400e-3 M} - \pu{6.39e−5 M} = \pu{0.336e-3 M}$$

Equilibrium constant

This is copied from the question, using the values calculated in this answer above and dropping the unit M because the standard state is 1 M:

$$\mathrm{K} = \frac{[\ce{FeSCN^2+}]}{[\ce{Fe^3+}][\ce{SCN^-}]}$$

$$\mathrm{K} = \frac{\pu{6.39e-5}}{\pu{} \pu{0.94e-3}\cdot \pu{0.336e-3}}$$

$$\mathrm{K} = 202$$