AP24 Q2 Class 23 (Collision Theory; Activation Energy)

Front

What is Collision Theory?

Back

Collision Theory states that for a reaction to occur, reactant particles must collide with sufficient energy and proper orientation.

Front

Define Activation Energy.

Back

Activation Energy is the minimum energy required for a chemical reaction to occur.

Front

What factors affect the rate of a chemical reaction?

Back

Factors include temperature, concentration of reactants, surface area, and the presence of catalysts.

Front

Explain the concept of the orientation factor in reactions.

Back

The orientation factor is a measure of how likely it is that colliding particles will be in the correct orientation to react.

Front

What is the significance of the rate-determining step in a reaction mechanism?

Back

The rate-determining step is the slowest step in a reaction mechanism, which determines the overall reaction rate.

Front

How does temperature influence reaction rates?

Back

Increasing temperature generally increases reaction rates because it increases the kinetic energy of particles, leading to more frequent and energetic collisions.

Front

What is the relationship between activation energy and reaction rate?

Back

Higher activation energy typically results in a slower reaction rate, as fewer particles have sufficient energy to overcome the barrier.

Front

What does a reaction profile illustrate?

Back

A reaction profile illustrates the energy changes during a chemical reaction, showing the activation energy and the enthalpy change.

Front

How does a catalyst affect activation energy?

Back

A catalyst lowers the activation energy of a reaction, allowing it to proceed more quickly without being consumed in the process.

Front

What is the enthalpy change in a chemical reaction?

Back

Enthalpy change is the difference in energy between the products and reactants, indicating whether a reaction is exothermic or endothermic.