CHEMISTRY COMMUNITY

Are Ice tables only for molarity? Or can we use them for partial pressures as well? I saw a question on Chemistry community about using partial pressures in ICE table but I thought it was only used for molarity. Thank you!

Ice tables can be used for both molarity and partial pressure because the concept is basically the same (Initial pressure, change in pressure and equilibrium pressure). For partial pressure you would just use Kp instead of Kw.

You can use it for both you just need to pay attention to what you are using when coming up with a final answer.

You can use it for both, but be careful when coming up with your final answer. Use Kp instead of Kw.

ICE tables can be used for questions of both reactant/product equilibrium partial pressure and concentration, as long as the correct K values are used.

Like said above, you can use both when calculating for your ICE table. The thing to keep in mind though is what the question asks for in the final answer. If in partial pressures, you may be asked to convert to molarity, or concentration (n/V).

ICE tables can be used for both pressure and molarity.

It can be used for both!

Unlike molarity which only limits us to use the ICE table using concentrations, partial pressures can allow for bar or atm as long as you are consistent with the units throughout.

ICE tables may be used for both cases. They are also helpful in comparing Q with K to check equilibrium.

ICE tables can be used for both, but I think there are specific cases in which if you are supposed to be solving for partial pressure, or given the units atm, then you might have to use the formula PV=nRT to convert to pressure.

they can also be used to acid and base