Question

explain what effect reducing volume of container will have on equilibrium in terms of PCl5

Answer 1

Suppose I initially have solid PCL5 in a container. Now it is heated
\[PCL5(s)rightarrowPCL3(g)+Cl2(g)\]
The solid gives rise to gases, meaning an increase in volume. Now some amount of air has to be pushed out, to make room for the increasing volume. If you've an open container, it'll be all right. But if it's closed, pressure will start building up, and the container may eventually burst.

Answer 2

i dont think thats the answer you give for equilibrium questions
the answer:
pcl5=pcl3 + cl2 . delta n = 1. so if you decrease volume,the reaction will go in the backward direction and more pcl5 will be formed from pcl3 and cl2

Answer 3

@Mani_Jha
It is a reversible reaction..

As the volume decreases, the pressure increases. To maintain the eqm position, you need to decrease the pressure, that is shifting the eqm to the side with less no. of mole of gas as reactants. From the equation, there is one mole of gas on left hand side, while 2 moles of gas on the right hand side. So the eqm will shift to the left so as to maintain the constant pressure and oppose the increase in pressure of the change