- Kp=Equilibrium constant in terms of partial pressure.
- Kc=Equilibrium constant in terms of concentration.
- Kx=Equilibrium constant in terms of mole fraction.
- Kn=Equilibrium constant in terms of number of moles.
- Kp and Kc are related as KP = KC (RT)∆n ...........................(eq 1)
Relationship between KP and Kn
...........................(eq 2) From ideal gas equation,PV=nRT
=>P=n(RT/V)
Where, n is the number of moles
So, PA =nA(RT/v), PB = nB(RT/V), PC =nC(RT/V) and PD =nD(RT/V)
Replacing equation 2 by the above value we get that,
[nC(RT/V)]c . [nD(RT/V)]d
Kp = -------------------------------------
[nA(RT/V)]a . [nB(RT/V)]b
nCc . nDd
= > Kp = -------------- . ( RT/V ) (c + d) – (a + b)
nAa. nBb
= > Kp = Kn . (RT/V) ∆n
= > Kp = Kn . (PT/nT) ∆n
∆n=number of gaseous moles of product – number of gaseous moles of reactant
Relation between Kp and Kx
From above (eq 2)
Partial pressure(P) = Mole fraction(x) . Total pressure(PT)
So, PA = xA . PT
PB = xB . P
PC = xC . PT
PD = xD . PT
Putting the values in whole equation:
Putting the values in whole equation:
( xC . PT )c . ( xD . PT )d
KP = ---------------------------------
( xA . PT )a . ( xB . PT )b
xCc . xDd
= -------------- PT(c+d) - (a+b)
xAa . xBb
= > KP = Kx (PT) ∆n
Q.Check your understanding.
N2O4(g)=2NO2(g) ,Calculate Kc and Kx for the given reaction for which Kp=0.157
Nyc
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But when they all will be equal
When number of moles in both product side and reactant side are equal,i.e. when ∆n=0, all the equilibrium constants become equal.
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I want to know relation between Kc an Kx .
Between Kp ,Kc, and Kx which has dimension ?
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All have a dimensions
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