Changing pressure

[Hailey Boehm 2H]

Why is there no change in the equilibria for the reaction 2 HD (g) = H2 (g) + D2 (g)? What are the rules for determining whether products or reactants will be favored in an instance where the pressure is increased?

[Christopher Tran 1J]

When pressure is increased, equilibrium will favor the side with less moles of gas. Since the reaction has two moles of reactant gas and two moles of reactant product, there is no change in equilibra.

[Miriam Sheetz 2B]

According to Le Chatelier's Principle, when the reaction undergoes a disturbance that does not involve a change in temperature, the reaction will adjust to minimize the effect of this disturbance. The reaction will move to favor the side with fewer moles of reactant/product. In this case, the moles are the same on both side so the rxn does not favor one or the other side.

[Erin Kim 2G]

When the pressure is increased, the volume is decreased, and the concentration is increased in a system, it will favor the side of the reaction with the less moles of gas. The vice versa is true as well. Because there are two moles of gas on both sides of the reaction, neither side will be favored.