Collision theory of concentration and partial pressure (Chemistry)

Question 1

If the concentration of reactant particles is increased

Answer 1

• This leads to an increase in the rate of collisions between reacting particles (only temporarily)
  • The forward reaction then increases
  • Corresponding to an increase in product and a decrease in reactant concentrations.
  • This leads to a decrease in the collisions of reactants (over time this occurs)
  • And Leads to an increase in product collisions
  • This leads to an increase in reverse reaction.
  • This cycle of concentration change, out of equilibrium, continues until the rate of the forward and reverse reactions are equal forming the new equilibrium.

The net effect of this change is a partial reduction of the imposed change (as it was initially increased)

Question 2

If the concentration of reactants is decreased

Answer 2

• The collisions between reactant particles decreases
  
  • This leads to a decrease in the reactant particles
  • Leading to an increase in the reverse reaction
  • This leads to an increase in the product collisions
  • Over time this leads to a decrease in product particles
  • Decreasing the product concentration
  • This leads to an increase in reactant concentration
  • Leading to an increase in reactant collisions
  • This leads to an increase in forward reaction
    This process repeats until a new equilibrium is reached.

Question 3

If imposed change of concentration increase occurs, what does Le Chatelier’s Principle predict?

Answer 3

The concentration will increase although a bit less than initially imposed.

Question 4

If imposed change of concentration decrease occurs, what does Le Chatelier’s Principle predict?

Answer 4

The concentration will decrease although a bit less of a decrease than initially imposed.