Answer:
See explanation
Explanation:
When the pressure is increased (or the volume reduced), the equilibrium will shift to the side of the smallest number of (gas)particles (numbers of moles). When the pressure is lowered, the particles can take up more space and the balance will shift to the side with the largest number of particles.
Consider the reaction N2O4 ⇄ 2NO
If we increase the pressure, the equilibrium will shift to the side with the smallest numbers. In this reaction, there is 1 mole consumed to produce 2 moles. This means the side of N2O4 is the side with the smallest number of particles. If the pressure will increase, the equilibrium will shift to the side of N2O4.
Consider the reaction N2(g) + 3 H2(g) ⇌ 2 NH3(g)
If we increase the pressure, the equilibrium will shift to the side with the smallest numbers. In this reaction, there is 1 mole of N2 and 3 H2 consumed to produce 2 moles of NH3. This means the side of NH3 is the side with the smallest number of particles. If the pressure will increase, the equilibrium will shift to the side of NH3.
When the left side has the same number of gas particles as the right side. The equilibrium will not change.
This shows that if we increase the pressure, the equilibrium will shift to the side with the smalles amount of gas particles, It doesn't always favor the product or reactants. But it is conserved.
