Question

Consider the reaction, which is exothermic as written, PCIs(g)% PCI3(g) + Cl2(g). Which of the following changes would result in the production of MORE C12(g)? I adding PCls(g) II. removing PCls(g) III reducing the volume of the container IV. removing PCls(g) V. increasing the temperature VI. increasing the volume of the container VII adding PCIs(g) VIII reducing the temperature IX. adding a suitable catalyst

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Answer 1

This question is based on the le Chataliers principle

According to which whenever a system is in equilibrium is disturbed

I will adjust itself in a way that the effect of the change will be cancelled or moderated.

a. In the above reaction if we add pcl3 (g) then according to le Chataliers principle eqillibrium will shifts toward left. And will decrease the production of cl2.

b. If pcl3 is removed then equilibrium will shifts towards right and production of cl2 will increase.

C. As we reduce the volume of the container then pressure will increase and shifts the equilibrium in the direction having less no. Of moles i.e. towards left and decrease the production of cl2.

D. On removing pcl5 the equilibrium will shifts towards left and decrease the production of cl2.

E. As it is an exothermic reaction which os favoured at low temperatures. On increasing the temperature production of cl2 will decrease. As equilibrium will shifts towards left.

F.As volume is increased of the container it means pressure is reduced and eqillibrium will shift in the direction having more number of moles of gases i.e. towards right. And increase the production of cl2.

G.On adding pcl5 equilibrium will shifts towards right, as pcl5 is consumed this side. Which will lead to the production of more cl2.

H. It is an exothermic reaction so on reducing the temperature equilibrium will shifts towards right and production of cl2 will increase.

I. Catalyst doesn't affects the equilibrium ,it only increases the speed of the reaction.

Thus 2,6,7,8 will increase the production of cl2.