Kc vs. Kp
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Kc vs. Kp
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?
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
Also, if you are given gas concentrations instead of partial pressures, it is ok to find Kc unless the problem states otherwise.
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Re: Kc vs. Kp
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.
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.
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
Kc and Kp are solved the same way, They are just denoted differently: Kc for concentration and Kp for pressure.
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
Yes, they are calculated the same way. You do not need to convert unless it is requested.
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Re: Kc vs. Kp
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).
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Re: Kc vs. Kp
Kc and Kp are calculated pretty much the same, the only difference you need to know is Kp is used for pressure.
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Re: Kc vs. Kp
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!
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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.
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.
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Re: Kc vs. Kp
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].
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Re: Kc vs. Kp
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!
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Re: Kc vs. Kp
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.
Last edited by Joanne Yuh 3I on Sat Feb 06, 2021 7:25 pm, edited 1 time in total.
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Re: Kc vs. Kp
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!
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Re: Kc vs. Kp
for Kc or Kp, the values should all be concentrations or partial pressures, respectively.
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Re: Kc vs. Kp
They are calculated similar to one another, and one can be used to convert to the other using the PV = nRT formula.
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Re: Kc vs. Kp
They are solved the same way, but, if given the information of one and the answer desires the other, you just have to convert.
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Re: Kc vs. Kp
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.)
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Re: Kc vs. Kp
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.
Re: Kc vs. Kp
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)
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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)).
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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!
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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!
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!
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Re: Kc vs. Kp
Kp and Kc are solved in the same way. The only difference is that they have different units (partial pressure and molar concentration).
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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.
You can convert partial pressures to concentration using the ideal gas equation. However, that would depend on the problem and information given.
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Re: Kc vs. Kp
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.
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.
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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)
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Re: Kc vs. Kp
it is the exact same way except for the units involved are different. The final outcome should be unitless though
Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
Hi,
Kc and Kp are solved the exact same way (P/R) however Kc refers to molar concentration whereas Kp refers to partial pressure.
Kc and Kp are solved the exact same way (P/R) however Kc refers to molar concentration whereas Kp refers to partial pressure.
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Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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)
Re: Kc vs. Kp
Yes, it’s calculated the same way—one is just for gases (pressure) and the other aqueous solutions (concentration).
Re: Kc vs. Kp
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.
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Re: Kc vs. Kp
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.
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