K vs KC
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K vs KC
For problems like 5I.13 in our textbook that asks us to refer to the table of Temperature to K constants on our textbook, which K are we supposed to use? One is "K" and the other has a "Kc." Some of these two K values are the same, but some are different, which would change our answer. Does anyone know how we would decide which K value to use?
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Re: K vs KC
Since Kc has to do with concentration, I would assume that for questions dealing with concentration, you would use Kc, and then use K otherwise? I'm not super sure myself but that is my guess.
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Re: K vs KC
Generally, Kc is used when referring to problems that are given in the form of molar concentrations. If I am correct, K is a more general term that is used to express an equilibrium constant.
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Re: K vs KC
They can mean the same thing, however K is used to represent the equilibrium constant. We use Kc when referring to concentration (molarity) and we can even use K to present partial pressure Kp (bar/atm)
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Re: K vs KC
K is just a generic equilibrium constant while Kc is for a reaction that uses its concentrations. In other words, it's just used for a reaction in the solution. For the most part, they should be the same because Kc is just more specific, but they are both equilibrium constants.
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Re: K vs KC
K is basically the umbrella term with Kc and Kp being the more specific terms. Kc is used when calculating concentration and Kp is used when calculating pressure
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Re: K vs KC
As other people have said, K is more of an overall term for the chemical equilibrium constant. Kc refers to the constant when it has been calculated using concentrations and Kp refers to the constant when it has been calculated using partial pressure. I'd suggest that when you are working on problems, you use either Kc or Kp, just so you get in the habit of associating the specific one to specific problems.
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Re: K vs KC
K is a generic umbrella term for the equilibrium constant whereas Kc is used specifically with equations dealing with concentrations.
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Re: K vs KC
The term K is just a general term that represents equilibrium constants. When you are trying to determine which K value to use, its important to pay attention to the state that the chemicals in the equation are present in, therefore determining what you would use as K. One example of this would be choosing Kp vs. Kc, where Kp would be used in equations that involve the gaseous state since it is measured as the partial pressure. On the other hand, you would use Kc when looking at aqueous states, since it measures the concentration (usually in molarity).
Re: K vs KC
Hi,
K represents the equilibrium ratio of products and reactants. When K is measured in concentration we call it Kc. This is still the same thing as K we have just specified that we are measuring in concentration. When K is measured in pressure we call it Kp. Also the same thing as K but measured in pressure. However, do not be confused because Kc =/= Kp when they are both numbers. Kc and Kp are two different ways to measure K.
K represents the equilibrium ratio of products and reactants. When K is measured in concentration we call it Kc. This is still the same thing as K we have just specified that we are measuring in concentration. When K is measured in pressure we call it Kp. Also the same thing as K but measured in pressure. However, do not be confused because Kc =/= Kp when they are both numbers. Kc and Kp are two different ways to measure K.
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Re: K vs KC
K is the general term for the equilibrium constant of a reaction. Meanwhile, Kc is the equilibrium constant that we use when dealing with concentrations expressed in molarity. There is also the term Kp, which we use when dealing with pressure.
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Re: K vs KC
Hey! K is the equilibrium constant, while Kc is a more specific type of equilibrium constant. Kc is specifically used when working with molar concentrations.
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Re: K vs KC
K is the general term to represent the equilibrium constant without units, whereas Kc is more specific in that it represents the equilibrium constant in units of concentrations (mol/L). They can be used interchangeably, but for the sake of clarity, I would recommend using Kc rather than K when dealing with concentrations.
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Re: K vs KC
KC refers to the equilibrium constant value that has to do with concentrations. K is just the general term for equilibrium constant
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Re: K vs KC
I think as a general way to approach this, you should look to see if the question mentions concentrations or pressure. This would help specify what K you're using. (if concentration then Kc or pressure than Kp) These can be converted from one another using P=n/v RT with n/v being concentration and P being pressure, so depending on what is given and what the answer is expected to be, you can convert between the two.
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Re: K vs KC
K is a more broad term to define the equilibrium constant and consists of Kc and Kp. Kc represents the equilibrium constant in concentrations (in terms of molarity (mol/L), whereas Kp represents the equilibrium constant in partial pressures. It's highly recommended to use either Kc or Kp depending on whether the problem uses concentrations or partial pressures just bc it's more specific!
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Re: K vs KC
K is generally used to refer to an equilibrium constant
Kc is an equilibrium constant when the concentrations of the substances at equilibrium are used in the calculation.
Kp is an equilibrium constant when the partial pressures of the substances at equilibrium are used in the calculation.
A small difference in the equations to find each value of K is the [ ] vs ( ). When calculating Kc, concentrations are in brackets; however, partial pressures when finding Kp are denoted in parentheses.
Kc is an equilibrium constant when the concentrations of the substances at equilibrium are used in the calculation.
Kp is an equilibrium constant when the partial pressures of the substances at equilibrium are used in the calculation.
A small difference in the equations to find each value of K is the [ ] vs ( ). When calculating Kc, concentrations are in brackets; however, partial pressures when finding Kp are denoted in parentheses.
Re: K vs KC
K aka Keq just refers to equilibrium constant, however Kc is specific to equilibrium constant in relation to concentrations and Kp is specific to equilibrium constant in relation to partial pressures.
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Re: K vs KC
K refers to an equilibrium constant. As for Kc, it is the ratio of equilibrium concentrations. Likewise, there is also Kp for equilibrium pressures, along with Ka and Kb for the equilibrium constant of acids and bases respectively. All represent a ratio of equilibrium products over equilibrium reactants.
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Re: K vs KC
Hi! I think my TA mentioned that in the textbook, they refer to Kp as K, and when we need to find Kc, they will write Kc instead.
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Re: K vs KC
I think Kc is specific to concentration only while K would be any type of equilibrium constant not only an equilibrium constant that's derived from equilibrium concentrations
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Re: K vs KC
K and Kc are practically the same. K is just the general equilibrium constant, and there are two types of equilibrium constants, Kc and Kp. Kc is to find the equilibrium constant when given or have substances that are at equilibrium concentrations.
Re: K vs KC
K, from my understanding, is a very loose term. It doesn't mean anything super specific, other than equilibrium. Whereas, Kc, is more specifically talking about concentration.
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Re: K vs KC
I'm pretty sure Kc is used for molar concentration while K is used for Equilibrium concentration. I just solve them the same way usually.
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Re: K vs KC
Like everyone has pointed out, I think K and KC are the same thing, but you can use KC more specifically for questions having to do with molar concentrations.
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Re: K vs KC
K is a general notation for equilibrium constant. Kc is the equilibrium constant used with regards to concentrations.
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