Consider the endothermic reaction

Question

2 NO(g) <-> N2(g) + O2(g)

-If I decrease the volume of the vessel and increasing the total pressure in the vessel, what direction will the equilibrium will shift? (left/right)
(I know that decreasing the volume would shift to produce less moles of gas, but the reaction has both 2 moles of gas left and right? What do I say in this case?)

-Added a catalyst, what direction will the equilibrium will shift? (left/right) and the concentrations of the products and reactants?
(I know catalysts don't affect equilibrium at all, but should I just write "N/A" for the direction and "no change" for NO, N2, and O2???)

Thanks in advance!

Answer 1

You're right. There are 2 mols gas on the left and 2 mols gas on the right; therefore, pressure has no effect.

You're right again on the catalyst. A catalyst will change the speed of a rxn but not the equilibrium point (that is, the rxn will get to equilibrium faster) but the end result is no changer in the equilibrium. Therefore, the rxn doesn't shift when a catalyst is added.