Question

A catalyst lowers the activation energy for both the forward and the reverse reactions in an equilibrium system, so it has no effect on the equilibrium position of a system. True False

Answer 1

Answer:

True.

Explanation:

• Catalyst increases the rate of the reaction without affecting the equilibrium position.

• Catalyst increases the rate via lowering the activation energy of the reaction.

• This can occur via passing the reaction in alternative pathway (changing the mechanism).

• The activation energy is the difference in potential energies between the reactants and transition state (for the forward reaction) and it is the difference in potential energies between the products and transition state (for the reverse reaction).

• in the presence of a catalyst, the activation energy is lowered by lowering the energy of the transition state, which is the rate-determining step, catalysts reduce the required energy of activation to allow a reaction to proceed and, in the case of a reversible reaction, reach equilibrium more rapidly.

• with adding a catalyst, both the forward and reverse reaction rates will speed up equally, which allowing the system to reach equilibrium faster.

• Kindly, see the attached image.

Answer 2

Answer:

The statement is true

Explanation:

When we add a catalyst to a system, both the forward and reverse reaction rates will speed up equally at the same time thereby allowing the system to reach equilibrium faster. But one thing that is very important to keep in mind that the addition of a catalyst has no effect on the final equilibrium position of the reaction because it only makes the reaction faster and nothing else.