8.1Rate of Reaction and Collision Theory

These flashcards cover key concepts and calculations related to the rate of reaction and collision theory as discussed in the lecture.

What is the rate of a chemical reaction?

The speed at which a chemical reaction takes place, measured in mol dm^-3 s^-1.

How is the rate of reaction calculated?

Rate of reaction = change in the amount of reactants or products (mol dm^-3) / time (s).

What is activation energy (E_a)?

The minimum energy that colliding particles must have for a collision to be successful in a chemical reaction.

What distinguishes an effective collision from an ineffective collision?

An effective collision has the correct orientation and sufficient energy, while an ineffective collision does not.

How does collision frequency relate to reaction rate?

An increase in collision frequency leads to a greater number of particles with energy greater than E_a, increasing the reaction rate.

What is a catalyst?

A substance that increases the rate of reaction without being consumed in the chemical reaction.

What effect does increasing concentration have on reaction rate?

Increased concentration raises the number of particles in a given volume, increasing collision frequency and thus the reaction rate.

How does increasing pressure affect the rate of reactions involving gases?

Increased pressure reduces volume, leading to more effective collisions and an increased reaction rate.

What happens to the concentration of reactants and products during a reaction?

The concentration of reactants decreases while the concentration of products increases as the reaction proceeds.

How can the rate of a reaction be calculated using a concentration-time graph?

The rate can be determined by calculating the change in concentration over time, or by drawing tangents at specific points.