Kc vs. Kp

[Shannon Moore 2L]

Do we solve for Kp in the same way that we solve for Kc? Do we need to convert between pressure and concentration if the equation is all gases?

[Ryan Laureano 3I]

You solve Kp the same way as Kc. If you wanted to convert between Kc and Kp you use Kp=Kc(RT)^(change in moles). You don't need to convert because kp uses partial pressures.

[Astha Sahoo 3I]

Yes! Like the other person above, you can change the PV = nRT, with n/V = [], to convert between the two. If you are switching between the two make sure to be careful because it's easy to make mistakes.

[Eliana Witham 2H]

Also, if you are given gas concentrations instead of partial pressures, it is ok to find Kc unless the problem states otherwise.

[Raashi Chaudhari 3B]

Hi!
To solve for Kc and Kp, it is the same set up of having products/reactants. The only difference is Kc uses the concentrations of the products over the concentrations of the reactants; while Kp uses the Pressure of the products over the pressure of the reactants. The same rules also follow with the stoichiometric coefficients; they are what the respective thing is raised to the power of.
Hope this helped.

[Shruti Kulkarni 2I]

You're right that solving for Kc and Kp is the same. Kp uses partial pressures while Kc uses concentrations. If you want to convert between the pressure to the concentration you can use PV = nRT, as n/V is concentration.

[Kayla Booker 1F]

Yes, you solve for Kp the same thing way as Kc

[MCalcagnie_ 1D]

Kc and Kp are solved the same way, They are just denoted differently: Kc for concentration and Kp for pressure.

[Krish_Ajmani_3J]

The only distinction between Kp is that it is uses partial pressures. Kc and Kp are, however, both calculated the same way. The species in the problems (gases or aqueous species) should help you determine which to use.

[Brian_Wu_3B]

Kp is calculated the same way as kc.

[Chudi Onyedika 3A]

Yes, they are calculated the same way. You do not need to convert unless it is requested.

[Keon Amirazodi 3H]

Yes, you do.

[Mehreen 3I]

Kp can Kc are calculated the same way! Kc is just for concentrations (molarity) and Kp is for partial pressures with gases (atm or bars).

[Jared Limqueco 3E]

Kc and Kp are calculated pretty much the same, the only difference you need to know is Kp is used for pressure.

[kristinalaudis3e]

Kc and Kp are calculated in the same way and both can be used for gases, but the only difference is that one is for partial pressures and one is for concentration. for whichever version you choose, make sure youre consistent with it the whole way through!

[Brianna Chen 3F]

Yes, they are solved the same way in which it is products over reactants! There is a formula that others have listed above if you want to convert from Kc to Kp or vice versa, but I like to look at the units provided to determine which one we should be solving for.

[Ivy Tan 1E]

Hi!
Yes, Kc and Kp are solved using the same formula. The only difference is that for Kp, you use the partial pressures for each gas and for Kc, you use the concentrations of each substance.

[Adam Bustamante 1I]

Kc and Kp are solved the same way! Kc is for concentration whereas Kp is for pressure, but both can be solved for using the setup: [products]/[reactants].

[Namita Shyam 3G]

Yep, Kc and Kp are solved the exact same way (products to the power of their coefficients over reactants to the power of their coefficients). For Kp, you just need to make sure that everything is in partial pressures, and for Kc, everything is in molar concentration. Also, don't include solids and liquids when your calculating!

[Joanne Yuh 3I]

You solve Kc and Kp the same way. You mostly only convert the concentration to pressure or pressure to concentration if the problem asks you to or there is an inconsistency in the units.

[Michelle Nguyen 3F]

Yes, you solve for Kc and Kp in the same way! Kc is for concentrations and Kp is for partial pressures. In terms of conversion, sometimes it would be helpful to use the Ideal Gas Law!

[Bai Rong Lin 2K]

They are calculated the same way!

[Nayra Gharpetian 3F]

yes we solve for kc the same way we solve for kp! :)

[Kaili Valenzuela 2B]

Yes Kp is calculated the same Kc is!

[Kathy_Li_1H]

Hi! Yes, we solve both the same way.

[derickngo3d]

for Kc or Kp, the values should all be concentrations or partial pressures, respectively.

[Kylie Joe 2A]

Both Kc and Kp are solved in the same way, they just involve different states

[aashmi_agrawal_3d]

Kc and Kp are solved for the same way.

[Sabrina Galvan 3J]

They are calculated similar to one another, and one can be used to convert to the other using the PV = nRT formula.

[Lizbeth Garcia 1F]

They are solved the same way, but, if given the information of one and the answer desires the other, you just have to convert.

[Anna Yang 1A]

Both are equilibrium constants and calculated the same way.

[Jacob Schwarz-Discussion 3I]

Kc and Kp are solved for in the exact same way. Kc uses the concentrations whereas Kp uses the pressures(make sure all the pressures have the same units(ex:atm,barr,etc.)

[Jose Miguel Conste 3H]

i believe any type of K is solved the same way

[Nicole Weinstein 3E]

Kc and Kp are solved the same way! Kc refers to concentrations or molarity, and Kp uses partial pressure values. Both find the equilibrium constant and the one you are trying to identify depends on the numbers you're given in their respective units.

[105743571]

Yes, you use the same equation and idea. If you want to convert molar concentration to partial pressure or the other way around, use the Ideal gas equation (PV = nRT)

[Helen Ringley 2E]

Yes! You use the same equation, its just different associated units.

[Joellen 1B]

Yes, you solve for Kc and Kp the same way. However, if you are given the concentrations, but it asks for Kp, you will need to use PV=nRT to convert it from concentration to pressure and vice versa if given the pressure when you need the concentration.

[Prithvi Raj 3E]

Yes, the method of solving for Kc and Kp are the same. You do the concentrations, or pressure, of the products over that over the reactants. To convert between the two, you use P=MRT where M is molarity and P is pressure.

[Ivy Vo Dis 1C]

Kc and Kp are calculated in the same format (products/reactants). However, these two values will use different inputs to calculate the equilibrium ratio. Kc will use the concentrations of the reactants and products to calculate K ([products]/[reactants). Meanwhile, Kp will use the partial pressures of the reactants and products to find equilibrium ratio ((Pressure of products)/(Pressure of reactants)).

[Anika Scott 3A]

Kc, Kp, K, Q, Qp, and Qc are all solved in the same way.

[Molly Smith 1J]

You solve for both in the same way. Just use Kp for gases (when all components are gas) and Kc for molar concentrations (they are aqueous a lot of the time). The ideology behind both is the same.

[Martha Avila 1I]

Hello. Yes, you will solve for Kc in the same way that you solve for Kp. The only difference is that for Kc you are dealing with concentration and with Kp you are dealing with pressure. You would still use the formula of products divided by reactants. This will either give you your Kc or Kp values but if asked to convert you would have to do so. Hope this helps!

[Aanjaneyaa]

They are both incredibly similar. The method between the two should be the same. The same type of thinking and the same formulas. The only difference is that Kc is for concentration and Kp is for partial pressure.

[Charlie Sjogren-Black]

Yes, the method for the two should be the same. However, when using Kp you must use partial pressures and when using Kc you must use concentrations. To transfer between the two use pv=nrt

[Yewon Jang 3K]

Kp uses the same equation as Kc. You use Kp when all the molecules in the equilibrium are in the gas phase and the units are given in bars/atms. You can use PV=nRT to convert between concentration and pressure.

[Benjamin Nguyen 1J]

Yes, Kc and Kp are calculated the same way.

[Myra Goraya Dis 2E]

You solve for Kp and Kc the same way, the only difference between the two are the units. Kc involves Molarity (moles/L) and Kp involved partial pressure (atm). The only thing to keep in mind is to make sure all the units are the same when plugging them into the equation.

[Samantha Loc 1B]

Hi there!
Like everyone else said, you pretty much solve for Kc and Kp the same way ([P]/[R]) except for Kc you use molar concentrations while for Kp you use pressure. You don't need to convert pressures to concentrations to solve for K, but if you wanted to you would use PV = nRT where (n/V) would be considered the concentration. Hope this helps!

[Ruben Adamov 1E]

Kp and Kc are solved in the same way. The only difference is that they have different units (partial pressure and molar concentration).

[Maggie Messer 1A]

You can solve Kp the same way that you solve Kc. The only difference between the two is the units. P is partial pressure while C is the molar concentration.

[Anthony_Rio_3K]

Is there another way to find partial pressures or is this the main/only way?

[Daniela G 2C]

Yes, solving for Kp requires the same steps as solving for Kc. The only difference is the subscript, p is for the unit partial pressure and c is for the unit concentration. Depending on the problem you might want to convert, but it is not necessary.

[Santiago Cortes 2J]

Yes you solve for Kc and Kp the same. The difference is that you would only use Kp when all the components are in the gas phase because it deals with partial pressures.
You can convert partial pressures to concentration using the ideal gas equation. However, that would depend on the problem and information given.

[Mario Prado 1K]

Hello,

Yes you would solve exactly the same way for both Kc and Kp the only difference is that Kc involves concentrations while Kp deals with partial pressures which when writing out the formula has you put the molecule as a subscript to the letter P to represent its a partial pressure.

Hope this helps.

[Jessica Li 1G]

Yes, they are calculated the same unless otherwise stated.

[cnyland]

Solving for Kp uses the same method as solving for Kc except for the fact that while solving for Kc, you should be using concentrations, and while solving for Kp you should be using partial pressures.

[Phoebe Ko 3E]

Yes, you would solve Kc the same way as Kp, except that you would calculate Kc with molar concentrations and Kp with partial pressures. Note that if a question specifically asks for Kc or Kp, you might have to convert the molar concentrations to partial pressures or vice versa using PV=nRT.

[Amanda Dankberg 1B]

you do solve kc the same way as kp but just be sure that everything is the same (either all kc or kp). The only time you need to convert is to make them all the same or if the question asks for something different than what is given (for ex the problem asks for kp but the concentrations are given). The equation to convert is Kp=Kc(RT)^(change in moles)

[Ivan Huang Dis 3B]

it is the exact same way except for the units involved are different. The final outcome should be unitless though

[HaleyC 2F]

Solving Kc and Kp is the same way they just are used differently. Kp is used when you are dealing with pressure and kc is used for concentrations.

[ajguerrero]

You would solve for them the same way its just that the difference is in the subscripts c, which is for concentration, and p, which is for pressure. you also would not need to convert since kp uses partial pressures

[Jessica Sun 2I]

The difference between Kc and Kp is that Kc is the equilibrium constant for molar concentration while Kp is the equilibrium constant for partial pressures.

[Michael 1G]

Kc and Kp are calculated in the same way. The only difference between the two is that Kc describes the molar concentration ratios of products and reactants and Kp describes product and reactant ratios in the gas phase using partial pressures.

[IA_1D]

From what I think Kc and Kp are solved the same way

[Arden Napoli 1E]

Hi,

Kc and Kp are solved the exact same way (P/R) however Kc refers to molar concentration whereas Kp refers to partial pressure.

[Amy Huynh 1B]

The way to solve for Kc and Kp is essentially the same. We would find Kc or Kp depending on what the problem gives us--Kc if they give us concentrations and Kp if they give us partial pressures. I don't think we need to convert anything to concentration or partial pressure unless it is stated in the problem that Kc or Kp is preferred over one or the other.

[Kaitlyn_Urquilla_1I]

Hi! Yes, you solve for Kc the same way you do for Kp.

[Alice Weber 3I]

Hi, Kp is calculated the same way as Kc.

[Uma Patil 2A]

Kc and Kp take the same forms. If we have all gases, we be using partial pressures of each gas in our calculation instead of concentrations. If for whatever reason you need to convert from partial pressure to concentration, you can use the ideal gas law (PV = nRT ==> n/V = P/RT)

[205769933]

Yes, it’s calculated the same way—one is just for gases (pressure) and the other aqueous solutions (concentration).

[Ally M]

They are solved the same way expect Kp is used when you are dealing with pressure and kc is used for concentrations, and you will obviously be dealing with different units.

[Aneesha_Nema_3C]

Yes, they're both solved in the same way. Just remember that Kp is for pressure and Kc is for molar concentration so make sure you're staying consistent with the values you're using to solve the problem.