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A certain volume of O2 gas is kept in a cylinder with a movable piston. If all the O2 molecules present in that cylinder get converted to O3 molecules at the same temperature and pressure, will you observe any change in the system?
Calculate the percentage change if any change takes place.
Justify your answer with appropriate reasons.

Solution:
3O2(g) → 2O3(g)
Since 3 moles of oxygen gives 2 moles of ozone.
At the same temperature and pressure, the volume of gas decreases.
If the volume of oxygen is v ml
the volume of ozone formed will be 2x3 ml
Decrease in volume=x - 2x3=x3 ml
%Decrease in volume=x3x×100% = 33.3%

 

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According to the kinetic theory of gases, yes of course there will be more collisions at a lower volume but pressure is a consequence of a force over the walls of the container, the mean sum of all collisions on the wall per unit of time do represent a net force and this force per unit of area is pressure.

The mean kinetic energy of the mass of gas that crashes against the walls is (KE)= (1/2)mv^2 and its derivative is the mean momentum =mv, following this route if thought we get again the derivative as a function of time of this momentum d(p)/dt = mdv/dt is mean force as dv/dt =a so (F)= ma so if this mass of gas m is that assigned to a unit of area A then the mean pressure if this mass is (P )= (F)/A.
Thus the percentage will be 33.33

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