A catalysta)Increases the average kinetic energy of reacting moleculesb)Increases the activation energyc)Alters the reaction mechanismd)Increases the frequency of collisions of reacting speciesCorrect answer is option 'D'. Can you explain this answer?

Question

Answer

In terms of the collision theory, increasing the concentration of a reactant increases in the number of collisions between the reacting species per second and therefore increases the reaction rate. Consider the reaction between hydrochloric acid and zinc metal

Answer

3

Answer

Ans is d because catalyst increases rate of formation of product by increasing frequency of collision of reacting species and by decreasing activation energy .

Answer

Explanation:

A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. It achieves this by providing an alternative reaction pathway with a lower activation energy. The correct answer to the given question is option 'D', which states that a catalyst increases the frequency of collisions of reacting species. Let's understand why this is the correct answer.

Collision Theory:
In order for a chemical reaction to occur, particles must collide with each other with sufficient energy and proper orientation. This concept is known as the collision theory. The rate of a reaction depends on the frequency of these collisions and the fraction of collisions with sufficient energy to overcome the activation energy barrier.

Role of Catalyst:
A catalyst increases the rate of a reaction by providing an alternative reaction pathway with a lower activation energy. It does so by forming temporary intermediate compounds with the reactant molecules, which lowers the energy required for the reaction to occur. This lower activation energy allows a larger fraction of collisions to have sufficient energy to overcome the barrier and proceed to product formation.

Increasing Collision Frequency:
One of the key ways in which a catalyst increases the rate of a reaction is by increasing the frequency of collisions between the reacting species. Here's how it happens:

1. Adsorption: The reactant molecules or ions are adsorbed onto the surface of the catalyst. This adsorption weakens the existing chemical bonds within the reactants, making them more prone to react.

2. Surface Mobility: Once adsorbed, the reactant molecules have increased mobility on the catalyst surface. This allows them to move around and come into contact with other reactant molecules more frequently.

3. Orientation: The catalyst can also provide a favorable orientation for the colliding reactant molecules, increasing the likelihood of successful collisions leading to reaction.

4. Desorption: Finally, the product molecules are desorbed from the catalyst surface, freeing up the active sites for further reactions.

Conclusion:
In summary, a catalyst increases the frequency of collisions between reacting species by adsorbing them onto its surface and providing favorable conditions for successful collisions. This increased collision frequency, along with the lowered activation energy, results in an overall increase in the rate of the reaction.

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