Final answer:
The addition of a catalyst to the reaction of crystal violet decreases the activation energy and increases the rate of the reaction, without changing the equilibrium constant or altering the reaction order.
Step-by-step explanation:
When a catalyst is added to a reaction, such as the reaction of crystal violet, several important changes occur:
- The activation energy required for the reaction to occur is decreased. This is because the catalyst provides a new pathway for the reaction with a lower energy barrier.
- As a result of the lower activation energy, the rate of the reaction increases. This occurs because a greater proportion of reactant molecules have sufficient energy to overcome the reduced energy barrier and form products.
- Contrary to some beliefs, the addition of a catalyst does not change the equilibrium constant (Keq) of the reaction. The equilibrium constant is dependant on the relative energies of the reactants and products, which are not altered by the presence of a catalyst.
- The reaction order is also not affected by the catalyst. Reaction order is determined by the stoichiometry and mechanism of the reaction, not the activation energy.
To answer the student's question directly, a catalyst would result in a decrease in activation energy (a) and increase in the rate of the reaction (b), but it would not change the equilibrium constant (c) or alter the reaction order (d).