using Kp vs Kc
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using Kp vs Kc
If all the reactants and products are in the gas phase, do you have to use Kp? Or can you use Kc?
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Re: using Kp vs Kc
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.
Last edited by Charysa Santos 4G on Fri Jan 10, 2020 12:37 pm, edited 1 time in total.
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Re: using Kp vs Kc
*Kc can be used for when concentrations are being used, while Kp is more particular to partial pressures and is more specific to gases.
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Re: using Kp vs Kc
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.
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Re: using Kp vs Kc
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.
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Re: using Kp vs Kc
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
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Re: using Kp vs Kc
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.
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Re: using Kp vs Kc
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.
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Re: using Kp vs Kc
You can use both but as everyone else mentioned, make sure to pay attention if you are given atms or mols.
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Re: using Kp vs Kc
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.
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Re: using Kp vs Kc
In fact, you can use both. Table 5G.2 shows an example of how Kc works for gas reactions.
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