Define KP
 
 
 
KP
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For gaseous equilibrium systems we can use partial pressure of gases instead of concentration. Therefore,
"Equilibrium constant determined by using partial pressure
of gases in a gaseous
chemical equilibrium is denoted by Kp"
Consider a general reversible reaction :
aA(g) + b B(g) c C(g) + d D(g)
For the reaction Kp is
Kp = [PC]c[PD]d/[PA]a[PB]b
Where [P] = partial pressure of gas
RELATION BETWEEN Kp AND Kc
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We know that Kp and Kc are related to each other as:

Kp = Kc[RT]Dn
From above relation we conclude three results as follows.
1. If Kp=Kc
In this case there is no change in volume
For example:
H2 + I2 2HI
In this example volumes of products are equal to the volumes reactants.
2. If Kp>Kc
In this case reaction occur with the increase in volume.
For example:
2NH3 N2 + 3H2
In this example volumes of products are greater than the volumes reactants.
3.If Kp<Kc
In this case reaction occur with the decrease in volume.
For example:
2SO2(g) + O2(g) 2SO3(g)
In this example volumes of products are less than the volumes reactants.
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