Here we have to get the
of the reaction at 520 K temperature.
The
of the reaction is 1.705 atm
We know the relation between
and
is
, where
= The equilibrium constant of the reaction in terms of partial pressure,
= The equilibrium constant of the reaction in terms of concentration and N = number of moles of gaseous products - Number of moles of gaseous reactants.
Now in this reaction, PCl₃ + Cl₂ ⇄ PCl₅
Thus number of moles of gaseous product is 1, and number of moles of gaseous reactants are 2. Thus N = |1 - 2| = 1 mole
The given value of
is 4.0×10⁻²
The molar gas constant, R = 0.082 L. Atm. mol⁻¹. K⁻¹ and temperature, T = 520 K.
On plugging the values in the equation we get,
![K_{p} = 4.0 X 10^{-2}(0.082X520)^{1}](https://tex.z-dn.net/?f=K_%7Bp%7D%20%3D%204.0%20X%2010%5E%7B-2%7D%280.082X520%29%5E%7B1%7D)
Or,
= 1.705 atm
Thus, the
of the reaction is 1.705 atm