Given that Â
      Â
     Â
PCl3(g)Â Â Â Â
+      Cl2(g) ⇌
PCl5(g)Â Â Â Â Â Â Â Â Kp =
0.16
Initial           Â
    0.5
atm            Â
0.5 atm         Â
0.3 atm
At equilibrium     Â
0.5-x                 Â
0.5-x            Â
0.3+x
                 Â
Kp = (0.3+x)/ [ (0.5-x) (0.5-x)]
             Â
0.16 = (0.3+x)/ (0.5-x)2
          Â
On solving,
            Â
x = -0.217 atm
Therefore,
Equilibrium partial pressures are
PCl3 = 0.5-x = 0.5 - (-0.217) = 0.717 atm
Cl2 = 0.5-x = 0.5 - (-0.217) = 0.717 atm
PCl5 = 0.3+x = 0.3-0.217 = 0.083 atm
--------------------------------------------------------------
Given reaction reaction exothermic.
All exothermic reactions are favoured by decrease in temperature
i.e. forward reaction reaction is favourable ( Equilibrium shifts
to right)
Hence,
X Cl2 increases when    increase the
temperature
X Cl2 decreases when   decrease the
temperature
X Cl2 stays the same   increase the volume of the
container
          Â
 Â
