AP Chemistry Help !!?

Question

Consider the following balanced equation in which gas X forms gas X2.

2X(g) --> X2 (g)

Equal moles of X are placed in two seperate containers. One container is rigid so the colume cannot change; the other container is flexible so the volume changes to keep the internal pressure equal to the external pressure. The above reaction is run each container. What happens to the pressure and density of the gas inside each container as reactants are converted to products?



Detailed Please ! =]
Thanksss !

Answer 1

Since 2 moles of reactant becomes 1 mole of product and you indicate the reaction is not an equilibrium process; in the rigid container, the pressure will drop to 1/2 the original level after the reaction is complete and the density should be 1/2 the density that X2 would have been at the original pressure. The reaction in the flexible container will cause the container to collapse to 1/2 the original volume so the gas density should be the same as normal for gas X2 (at the pressure surrounding the container).