3 excessive clean up mathjax

I tried to do the question below and I want to make sure if I did correctly.

The question is:

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

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 15.0 mL + 15.0 mL = 30 mL$$\pu{15.0 mL + 15.0 mL = 30 mL}$$ to L and I got 0.03L$$\pu{0.03L}$$

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

Thirdly, I did the ICE chart

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

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

I tried to do the question below and I want to make sure if I did correctly.

The question is:

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

Firstly, I converted the total volume 15.0 mL + 15.0 mL = 30 mL to L and I got 0.03L

Secondly, I used the given 0.00450 mol and divided it by 0.03 L and I got 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 Kc at equilibrium

I got 1.53 for Kc but I am not sure if the whole process is correctly done. Please point out my mistakes, thank you very much.

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

2 Asker did not state that initial concentration for BC was 0, and end was 0.0450 mol, creating an entirely different problem.

I tried to do the question below and I want to make sure if I did correctly.

The question is:

Ions B and C react to form complex BC. If 15.0 mL of 1.00 M B is combined with 15.0 mL of 1.00 M C, 0.00450 moland our initial concentration of BC is 0, yet the end in equilibrium for complex BC is formed0. Determine00450 mol determine the equilibrium constant for this reaction.

Firstly, I converted the total volume 15.0 mL + 15.0 mL = 30 mL to L and I got 0.03L

Secondly, I used the given 0.00450 mol and divided it by 0.03 L and I got 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 Kc at equilibrium

I got 1.53 for Kc but I am not sure if the whole process is correctly done. Please point out my mistakes, thank you very much.

I tried to do the question below and I want to make sure if I did correctly.

The question is:

Ions B and C react to form complex BC. If 15.0 mL of 1.00 M B is combined with 15.0 mL of 1.00 M C, 0.00450 mol of complex BC is formed. Determine the equilibrium constant for this reaction.

Firstly, I converted the total volume 15.0 mL + 15.0 mL = 30 mL to L and I got 0.03L

Secondly, I used the given 0.00450 mol and divided it by 0.03 L and I got 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 Kc at equilibrium

I got 1.53 for Kc but I am not sure if the whole process is correctly done. Please point out my mistakes, thank you very much.

I tried to do the question below and I want to make sure if I did correctly.

The question is:

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

Firstly, I converted the total volume 15.0 mL + 15.0 mL = 30 mL to L and I got 0.03L

Secondly, I used the given 0.00450 mol and divided it by 0.03 L and I got 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 Kc at equilibrium

I got 1.53 for Kc but I am not sure if the whole process is correctly done. Please point out my mistakes, thank you very much.

1

# Determine the equilibrium constant for this reaction

I tried to do the question below and I want to make sure if I did correctly.

The question is:

Ions B and C react to form complex BC. If 15.0 mL of 1.00 M B is combined with 15.0 mL of 1.00 M C, 0.00450 mol of complex BC is formed. Determine the equilibrium constant for this reaction.

Firstly, I converted the total volume 15.0 mL + 15.0 mL = 30 mL to L and I got 0.03L

Secondly, I used the given 0.00450 mol and divided it by 0.03 L and I got 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 Kc at equilibrium

I got 1.53 for Kc but I am not sure if the whole process is correctly done. Please point out my mistakes, thank you very much.