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# Determine the equilibrium constant for this reaction

The question is:

Ions $$\ce{B}$$ and $$\ce{C}$$ react to form complex $$\ce{BC}$$. If $$\pu{15.0 mL}$$ of $$\pu{1.00 M}$$ $$\ce{B}$$ is combined with $$\pu{15.0 mL}$$ of $$\pu{1.00 M}$$ $$\ce{C}$$, and our initial concentration of BC is $$0$$, yet the end in equilibrium for complex $$\ce{BC}$$ is $$\pu{0.00450 mol}$$ determine the equilibrium constant for this reaction.

Firstly, I converted the total volume $$\pu{15.0 mL + 15.0 mL = 30 mL}$$ to L and I got $$\pu{0.03L}$$

Secondly, I used the given $$\pu{0.00450 mol}$$ and divided it by $$\pu{0.03 L}$$ and I got $$\pu{0.15 M}$$ for BC

Thirdly, I did the ICE chart

After that, I used the quadratic formula to solve for $$x$$ and calculate the concentration for each substance, as well as getting the $$K_\mathrm{c}$$ at equilibrium

I got $$1.53$$ for $$K_\mathrm{c}$$ but I am not sure if the whole process is correctly done. Please point out my mistakes