Collision Theory and Reaction Rates

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

How does temperature affect reaction rates?

Back

Increasing temperature increases the kinetic energy of particles, leading to more frequent and effective collisions, thus increasing the reaction rate.

Front

What is the effect of concentration on reaction rates?

Back

Higher concentration increases the number of reactant particles in a given volume, leading to more frequent collisions and a higher reaction rate.

Front

Why does increasing surface area speed up reactions?

Back

Increasing surface area allows more particles to be exposed and available for collisions, leading to an increased rate of reaction.

Front

What is activation energy?

Back

Activation energy is the minimum energy required for reactants to collide and form products.

Front

How does particle size influence reaction rates?

Back

Smaller particle size increases the surface area available for reaction, leading to more collisions and a faster reaction rate.

Front

What is the relationship between reaction rate and the speed of reaction?

Back

The reaction rate is a measure of how quickly reactants are converted into products, which is directly related to the speed of the reaction.

Front

What role do catalysts play in chemical reactions?

Back

Catalysts increase the rate of a reaction by lowering the activation energy without being consumed in the process.

Front

How does pressure affect reaction rates in gases?

Back

Increasing pressure in gas reactions decreases the volume, leading to more frequent collisions and an increased reaction rate.

Front

What is the effect of a decrease in temperature on reaction rates?

Back

Decreasing temperature reduces the kinetic energy of particles, leading to fewer collisions and a slower reaction rate.