Question

What is catalysis and what does a catalyst do to the activation energy of a reaction, and to the rate of the reaction. Does a catalyst change the nature of the products of the reaction? If a reaction is in equilibrium, does adding a catalyst shift the equilibrium?

Answer 1

Catalysis is the process by which a catalyst lowers the activation energy of a chemical reaction, thus increasing the reaction rate without changing the nature of the products. A catalyst does not shift the position of a reaction at equilibrium but enables the system to reach equilibrium more quickly.

Step-by-step explanation:

What is Catalysis?

Catalysis refers to the process by which a catalyst increases the rate at which a chemical reaction occurs. A catalyst facilitates a chemical reaction without undergoing any permanent chemical change itself. It works by providing an alternative reaction pathway with a lower activation energy (Ea), which is the energy required to initiate the reaction. This lower activation energy means that more reactant molecules can effectively collide and react at a given temperature, thereby speeding up the reaction rate.

Effect on Activation Energy and Reaction Rate

The presence of a catalyst in a chemical reaction results in a lower activation energy barrier. This, in turn, means that a greater percentage of reactant molecules have enough energy to overcome this barrier and form products. Consequently, the reaction rate is increased since the reaction can proceed faster.

Does a Catalyst Change the Nature of the Products?

A catalyst does not affect the energy of the reactants or the products, nor does it alter the overall thermodynamics of the reaction. Therefore, it does not change the nature of the products of the reaction.

Adding a Catalyst to a Reaction in Equilibrium

When a reaction is in equilibrium, adding a catalyst will not shift the equilibrium position or alter the concentrations of reactants and products at equilibrium. Instead, it will increase the rate at which equilibrium is reached by speeding up both the forward and reverse reactions equally.

Answer 2

Answer in explanation

Step-by-step explanation:

A catalyst is a substance that alter the rate of a chemical reaction. It either speeds up the rate of the chemical reaction or slows down the rate of the chemical reaction. Hence, we say a catalyst can either work positively or negatively.

A catalyst will bring down the value of the activation energy. It reduces the minimum amount of energy needed for the reaction to kickstart. Hence we say it tends to create an alternative pathway for the chemical reaction to proceed.

When it speeds up the rate, it is otherwise known as a positive catalyst, otherwise it is a negative catalyst.

A catalyst does not have any business with the nature of the products or the reactants. Its work is simple, either hasten or slow down the rate of a chemical reaction.

A catalyst has no effect On the equilibrium position of a chemical reaction. This is to say its addition or subtraction has no effect on the position of a chemical reaction