Question

Which part(s) of the reaction 2 HD(g) ⇀↽ H2(g) + D2(g) will be favored by an increase in the total pressure (resulting in compression)?

Answer 1

Neither side is favored

Step-by-step explanation:

In a reaction at equilibrium in which reactants and products are gases, pressure is a factor that produces a shift of the equilibrium position. When the pressure is increased, the equilibrium is shifted to the side of the reaction with a fewer moles. In this reaction:

2 HD(g) ⇀↽ H₂(g) + D₂(g)

There is the same number of moles on both sides:

reactants side: 2 moles HD

products side: 1 mol H₂ + 1 mol D₂ = 2 moles

Therefore, the equilibrium position will not change.