3 excessive clean up mathjax
source | link

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

enter image description here

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

enter image description here

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

enter image description here

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

enter image description here

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

enter image description here

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

enter image description here

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

    Tweeted twitter.com/#!/StackChemistry/status/442927631663890432
2 Asker did not state that initial concentration for BC was 0, and end was 0.0450 mol, creating an entirely different problem.
source | link

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

enter image description here

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

enter image description here

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

enter image description here

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

enter image description here

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

enter image description here

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

enter image description here

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
source | link

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

enter image description here

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

enter image description here

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.