ICE Table Practice Problems - Initial Concentration, Equilibrium Concentration, Kc (Part 1)

[@lily2341]

this is so helpful!!! thank you so so much from the bottom of my heart.

[@danpireocean4802]

look at conquer chemistry man, so inspirational

[@arabellajennings6058]

took 10 minutes to explain what my prof couldn't for 3 hours

[@Jackson-ms2qq]

I second that

[@kaytlint3165]

Thank you for taking the time to make this video-- it is truly SO helpful

[@milko5143]

Nah this is actually legendary best vid on this topic

[@akosg4057]

I would like to thank you, this has saved my chemistry grade

[@CRGLightning-YT]

Thank you! This video helped me understand ICE tables.

[@gdgshevvvdvdgg4428]

I been looking for a video like this for so long 🙏🏾 thx

[@techBRO1024]

So clear and understandable, thank you!!!

[@ChipangoMuti-c2n]

It has helped me continue doing the good work

[@gabrielle-lk8pm]

thank you :-)

[@sci8]

Great practice problems, thanks for the video.

[@TheDallasDwayne]

You are the chemistry guru!

[@mohfa1806]

Thank you for your great educational videos...i have a question please : our chemistry teacher told us that in the ICE we use only number of moles , but in your lesson here you used concentrations , so in the ICE table we have the choice of using number of moles or concentrations ?...thank you again.

[@aliwoolf617]

I know I’m not the KZbinr, but I thought I’d help out. I’m pretty sure you have to use the concentrations. Not sure why your teacher said moles but in every example I’ve done for studying for my test it’s been the concentration (also my teacher said concentrations as well!). Hope this helps!

[@kaitlynnags1384]

The ICE table stands for Initial (concentration) Change (in concentration) and (concentration at) Equilibrium. In the ICE table, you multiple the number of moles by the concentration if it isn't a 1:1 mole ratio. I hope I explained this well!

[@gino2026]

ICE tables can be used for Concentration, Pressure, Moles, or Molar fractions as long as you commit to using one of them. When you select one of the four properties, the procedure is exactly the same, but you'll obtain as a result the equilibrium values of the selected property. For example, in problem 2, if you follow the procedure with moles instead of concentration, the units of "x" will be moles, and you'll obtain the equilibrium number of moles for species A,B,C,D. Those can be used to calculate both the total concentration C = (NA+NB+NC+ND)/V, and the equilibrium molar fractions of all species (XA,XB,XC,XD). Then, you can calculate Kx = (XC)^c (XC)^d / [(XA)^a (XB)^b]. Finally, you can calculate Kc using the following relationship: Kc = Kx(C)^Δn Alternatively, you could also multiply each molar fraction by the total concentration (C) to calculate each equilibrium concentration (CA,CB,CC,CD), and substitute those values into the expression of Kc to calculate it.

[@mohfa1806]

@@gino2026 thank you for your reply...it was really helpfull

[@jacobkasalika9569]

So helpful

[@amadeusm8590]

thanks boss for the thick answer

[@victoria-b3b8p]

dude bless you

[@Obaid-Ur-Rahman342]

Thank you so much

[@oreofe8266]

Thank you!

[@CaptainRowsdower]

You are awesome!

[@reryray7072]

Thank youuuuu❤❤❤❤

[@peytonf4416]

Thanks so much, but how to I cross multiply?

[@bagundolancis7929]

where does 0.5 came from?

[@belieste]

based video thanks this really helps

[@allheart4uministries285]

Thank you so much!!!😭

[@sliderulelover]

I hate it when instructors already start with a balanced equation. It's a much more fun problem when we students have to first balance the equation. Stop already with the balancing equations! We're not idiots.

[@gino2026]

If someone were to balance the same reaction differently but equivalently, for example: 1/2 Br2 + 1/2 Cl2 BrCl Kc1 Or Br2 + Cl2 2BrCl Kc2 Then the value of Kc2 and Kc1 would be different, since Kc2 = Kc1 ^ 2 So unless the instructor demands some specific balancing rule (like always using the lowest whole numbers for coefficients), it's important to know what the balanced equation looks like for equilibrium problems.