Rate or reaction 💥

Rate of reaction

The change in amount or concentration of reactants or products per unit time

What are factors that affect the rate of reaction?

Nature of reacting substance, surface area, concentration, temperature and a catalyst

Collision theory

A model that explains reaction rate as a result of particles colliding with a certain minimum energy

A catalyst

A substance that increases the rate of reaction but remains unchanged at the end of the reaction

What are the requirements that a reactant must have to have an effective collision?

correct or orientation of particles and enough sufficient energy

Explain how the nature of reactant affects the rate of reaction

Metals down the group are more reactive and across the period. They are less reactive nonmetals are more reactive across the period and reactivity decreases down the group.

How does surface area increase rate of reaction?

Larger the surface area more particles are exposed to other reactants and more particles are available for collision. The number of collisions or frequency per second will increase and there’s gonna be more effective collision and the overall rate of reaction will increase

how does temperature increase the rate of reaction?

When temperature increases the kinetic energy also increases and particles will move faster and more collisions per second will occur and more collisions will have enough energy to react and the number of effective collision with increases resulting in the overall rate of reaction increasing

How does concentration increase rate of reaction?

When the number of constitution of particles increases they’re gonna be more particles exposed to their reactant and more collisions will occur per second and more effective collisions will occur resulting in the overall increase of rate of fraction

What is bond energy?

Amount of energy needed to break one mole of a particular type of bond

Bond lengths

The average distance between the nuclei of two bonded atoms

Activation energy

The minimum energy needed for the reaction to take place

Activated complex

A high energy, unstable transition state between the reactants and the products

Heat of reaction

The net change of chemical potential energy of the system

Exothermic

Reaction which transforms chemical potential energy to thermal energy

Endothermic

A reaction which transfers thermal energy to chemical potential energy