derive relationship between Kp and Kc

Let us assume a general reaction:

For this reaction,

We know,

Where,

M = molarity

 

Therefore,

Now,

Therefore,

Where,

 

  • 68

 Hi,

Follow the given steps to derive the relationship between Kp and Kc.


thubs up plz !

  • 27

  • Relationship between Cp and Cv for an ideal gas

Cp  Heat capacity at constant pressure

C Heat capacity at constant volume

At constant volume: qCvΔT = ΔU

At constant pressure: qpCpΔT = ΔH

For a mole of an ideal gas:

ΔH = ΔU + Δ(pV)

ΔU + Δ(RT)

ΔU + RΔT

∴ΔH = ΔU + RΔT

⇒ CpΔT = CvΔT + RΔT

⇒ Cp = Cv + R

⇒ Cp − Cv = R

  • 2

 

"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.

  • 8

 sry prvious answer is not correct it is my mistake

  • 1
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