using Kp vs Kc

[Clarice Chui 2C]

If all the reactants and products are in the gas phase, do you have to use Kp? Or can you use Kc?

[Charysa Santos 4G]

If all of the reactants and products are in the gas phase, then you must use Kp if only the partial pressures are given. Kc* is used for concentrations, and is thus used when the reactants and products are in the aqueous phase. I think it depends on what you are given.

[Maia_Jackson_2C]

I think you should get the same number for both, but I'm not entirely sure.

[Charysa Santos 4G]

*Kc can be used for when concentrations are being used, while Kp is more particular to partial pressures and is more specific to gases.

[Katie Kyan 2K]

I think for an equation involving gases, either Kp or Kc can be used since you can convert from one to the other using the Ideal Gas Law.

[Hannah Pham]

Kp is for partial pressure, so when your products and reactants are in the gas phase. Kc is for concentration. However, for gases, you can use either Kc or Kp and just convert using the Ideal Gas Law.

[Sally Qiu 2E]

you would use Kp if you are given the partial pressures.

[Kylie Lim 4G]

Kp is used when you have the partial pressures of a gas, and Kc is used for concentration which can be found using PV=nRT

[Anna Heckler 2C]

You can convert between Kp and Kc using the ideal gas law. Kp is used for partial pressures of gases, whereas Kc is used for concentrations.

[lauraxie2e]

You use Kp

[Jaci Glassick 2G]

Both can be used. Kc can be used when dealing with concentrations while Kp can be used when dealing with partial pressures. I believe the values will be the same.

[ayushibanerjee06]

You can use both but as everyone else mentioned, make sure to pay attention if you are given atms or mols.

[Vivianvelazquez_1J]

If all the reactants and products are in the gas phase you would use Kp. Kp is for partial pressure when your reactants and products are in the gas phase. While Kc is for when concentrations are being used.

[Nuoya Jiang]

In fact, you can use both. Table 5G.2 shows an example of how Kc works for gas reactions.