A catalyst affects the rate of a reaction by providing an alternative reaction pathway with a lower activation energy. This means that more of the reactant particles will have enough energy to undergo the reaction, thus increasing the rate of the reaction.

Here's a step-by-step explanation:

1. A catalyst is introduced to a reaction. This catalyst is not consumed in the reaction, meaning it can be used repeatedly.

2. The catalyst provides an alternative reaction pathway with a lower activation energy. Activation energy is the minimum amount of energy required for a reaction to occur.

3. Because the activation energy is lower, more reactant particles will have enough energy to react. This increases the number of successful collisions between reactant particles.

4. As a result, the rate of the reaction increases. The catalyst speeds up the reaction, but does not affect the position of the equilibrium or the enthalpy change of the reaction.

An example of a specific acid-catalysed reaction is the est

Question

A catalyst affects the rate of a reaction by providing an alternative reaction pathway with a lower activation energy. This means that more of the reactant particles will have enough energy to undergo the reaction, thus increasing the rate of the reaction.

Here's a step-by-step explanation:

1. A catalyst is introduced to a reaction. This catalyst is not consumed in the reaction, meaning it can be used repeatedly.

2. The catalyst provides an alternative reaction pathway with a lower activation energy. Activation energy is the minimum amount of energy required for a reaction to occur.

3. Because the activation energy is lower, more reactant particles will have enough energy to react. This increases the number of successful collisions between reactant particles.

4. As a result, the rate of the reaction increases. The catalyst speeds up the reaction, but does not affect the position of the equilibrium or the enthalpy change of the reaction.

An example of a specific acid-catalysed reaction is the est

Knowee AI · Accepted Answer

A catalyst affects the rate of a reaction by providing an alternative reaction pathway with a lower activation energy. This means that more of the reactant particles will have enough energy to undergo the reaction, thus increasing the rate of the reaction.

Here's a step-by-step explanation:

1. A catalyst is introduced to a reaction. This catalyst is not consumed in the reaction, meaning it can be used repeatedly.

2. The catalyst provides an alternative reaction pathway with a lower activation energy. Activation energy is the minimum amount of energy required for a reaction to occur.

3. Because the activation energy is lower, more reactant particles will have enough energy to react. This increases the number of successful collisions between reactant particles.

4. As a result, the rate of the reaction increases. The catalyst speeds up the reaction, but does not affect the position of the equilibrium or the enthalpy change of the reaction.

An example of a specific acid-catalysed reaction is the est

How does a catalyst effect rate of a reaction? Give an example of specific acid catalysedreaction.

Question

Solution

Similar Questions

Upgrade your grade with Knowee